Honor Biology Remember that the greater the concentration of hydrogen ions, the lower the pH of a solution. How do you suppose the pH of the solution in the thylakoid space compares with the pH of the solution in the stroma? What is responsible for the difference? Monday, December 6, 2010 at 4:02pm by Pam
Honors Biology - URGENT!!! Remember that the greater the concentration of hydrogen ions, the lower the pH of a solution. How do you suppose the pH of the solution in the thylakoid space compares with the pH of the solution in the stroma? What is responsible for the difference? Wednesday, December 8, 2010 at 8:15am by Brenda
chemistry I am having trouble with how to approach this problem. I have the solution but can't figure out how to get it. How many moles of NaOH must be added to 1.0 L of 2.0M HC2H3O2 to produce a solution buffered at each pH? a) pH=pKa b)pH=4 c)ph=5 Monday, April 12, 2010 at 9:18pm by heather
Chemistry I am having trouble with how to approach this problem. I have the solution but can't figure out how to get it. How many moles of NaOH must be added to 1.0 L of 2.0M HC2H3O2 to produce a solution buffered at each pH? a) pH=pKa b)pH=4 c)ph=5 Monday, April 12, 2010 at 6:42pm by Larry
chemistry Q.1 What will be the pH at the equivalence point during the titration of a 100 ml 0.2M solution of CH3COONa with 0.2M of solution of HCl?(Ka = 2*10^-5) Q.2 Aniline behaves as a weak base.When 0.1M,50ml solution of aniline was mixed with 0.1M,25ml solution of HCl the pH of resu... Saturday, March 27, 2010 at 6:47am by gaurav
chemistry Disadvantage of using pH indicators for what? For titrations it is that not all indicators change at the equivalence point pH. If for determining the pH of a solution, it is because most pH indicators have a pH range of about 2 pH units which isn't very close if you want t... Wednesday, April 29, 2009 at 8:23pm by DrBob222
chemistry-confirm please Only a chemist can be trusted with the combination to the safe containing a ton of money. The combination is the pH of solution A, followed by the pH of solution C. (for example: is the pH of solution A is 3.47 and the pH of solution C is 8.15 the combination to the safe is 3-... Sunday, May 25, 2008 at 2:51pm by Tom
Chemistry The pH of a solution is 11.30. In order to find the concentration of H+, wouldn't I simply take the pH of the solution and plug it into the formula 10^-pH? Wednesday, September 16, 2009 at 11:21pm by Anonymous
chemistry A. Strong Base 1.) What is the concentration of a solution of KOH for which the pH is 11.89? 2.) What is the pH of a 0.011M solution of Ca(OH)2? B. Weak Acid 1.) The pH of a 0.060M weak monoprotic acid HA is 3.44. Calculate the Ka of the acid. 2.) The pH of 0.100M solution of ... Thursday, January 20, 2011 at 3:37am by jaycab
Chemistry A buffer solution of volume 100.0 mL is 0.150 M Na2HPO4(aq) and 0.100 M KH2PO4(aq). Refer to table 1. (a) What are the pH and the pH change resulting from the addition of 80.0 mL of 0.0500 M NaOH(aq) to the buffer solution? pH pH change (include negative sign if appropriate) (... Tuesday, March 16, 2010 at 11:52pm by Trixie
Chemistry A 100 milliliter sample of 0.100-molar NH4Cl solution was added to 80 milliliters of a 0.200-molar solution of NH3. The value of Kb for ammonia is 1.79 x 10^-5. (a) What is the value of pKb for ammonia? (b) What is the pH of the solution described in the question? (c) If 0.200... Monday, April 26, 2010 at 8:58pm by Nicole
Chemistry A 100 milliliter sample of 0.100-molar NH4Cl solution was added to 80 milliliters of a 0.200-molar solution of NH3. The value of Kb for ammonia is 1.79 x 10^-5. (a) What is the value of pKb for ammonia? (b) What is the pH of the solution described in the question? (c) If 0.200... Monday, April 26, 2010 at 8:49pm by Nicole
chemistry Solution A has a pH of 5, and solution B has a pH of 11. If equal amounts of A and B are mixed, is the resulting solution acidic or basic? Tuesday, June 22, 2010 at 9:45pm by Jim
biology if a solution has a pH of 4 mix to a solution that has a pH of 9 what will be the pH of the mixed solution? will it be acidic or base? please show me how to calculate it.please i need the answer before tomorrow morning. thank you so much. I had been to other sites but i didn&#... Tuesday, October 20, 2009 at 10:37pm by heather
chemistry which solution has the highest concentration of hydroxide ions? a ph=7.93 b ph=12.59 c ph=7.00 d ph=9.82 e ph=3.21 i know the answer is 7 but why is it seven? would it be different if it said hydronium ions? Saturday, December 11, 2010 at 1:07pm by jessie
chemistry Here are 2 questions I worked out, but need them checked. Also, can't get answer to another question correct unless question 1 is correct. Would you check the first 2 and help me with the third? 1) What is the pH of a 0.05 M solution of TRIS acid (pka = 8.3)? My answer: I ... Saturday, February 2, 2008 at 1:38pm by alan
chemistry lab Here are 2 questions I worked out, but need them checked. Also, can't get answer to another question correct unless question 1 is correct. Would you check the first 2 and help me with the third? 1) What is the pH of a 0.05 M solution of TRIS acid (pka = 8.3)? My answer: I ... Saturday, February 2, 2008 at 11:31pm by ryan
Chemistry Posted by Hannah on Saturday, April 18, 2009 at 3:05pm. Find the pH of a 0.010M solution of NH4ClO4 and the pH of a 0.010M solution of NH4C2H3O2. Responses * chemistry - Anonymous, Saturday, April 18, 2009 at 3:36pm after finding the ph of the corresponding ions in these two q... Saturday, April 18, 2009 at 3:43pm by Anonymous
Chemistry A potassium hydroxide solution has a pH of 12.90. Enough cid is added to react with half of the OH- ions present. What is the pH of the resulting solution? Assume that the products of the neutralization have no effect on pH and that the amount of additional water produced is n... Tuesday, May 4, 2010 at 7:37pm by Alexa
Chemistry Captain Kirk, of the Starship Enterprise, has been told by his superiors that only a chemist can be trusted with the combination to the safe containing the dilithium crystals that power the ship. The combination is the pH of Solution A described below, followed by the pH of S... Tuesday, May 27, 2008 at 7:38pm by Tom
Chemistry If one were to mix 200.0 mL of an HCl solution that had a pH of 3.00 with 200.0 mL of an NaOH solution that had a pH of 10.00, what would be the pH of the final solution? Can you show me the steps please so that I can apply to questions that ask for the same type of solving? t... Thursday, December 16, 2010 at 9:42pm by Anonymous
chemistry A pH glass/calomel electrode was found to develop a potential of -0.0390 V when used with buffer of pH 5.52. With an unknown solution, the potential was -0.360 V. Calculate the pH of the unknown solution Wednesday, November 17, 2010 at 1:37pm by Nikki
pH???+chem! 7. A few drops of bromothymol blue indicator are placed into 250 mL of 0.20 mol/L HCl(aq). A sample of 1.8 g of NaOH(s) is then dissolved into this solution. The final colour of the solution is predicted to be How can I do this one? What is the pH of the HCl solution? THen, di... Friday, August 4, 2006 at 7:48pm by Bobby
college chemistry Suppose you have a 0.200 M solution of the nitrogen-containing weak base NX. Suppose you wish to titrate 25 mL of this 0.200 M NX solution with a 0.100 M solution of the strong acid HNO3. Given that the Kb value of NX is 6.50x10-5, complete each of the following: a) What volum... Wednesday, April 21, 2010 at 5:58pm by Aubree
chemistry if the pH of a half-neutralized acid solution is 5.4, how would you find the [H+] of the the solution. There is 1.0 g of L-ascorbic acid which was dissolved in 100 ml of water. That solution was split in two and 50 ml of the solution was titrated with 0.2 M NaOH (13 ml NaOH). ... Thursday, April 17, 2008 at 3:04pm by tom
CHEMISTRY Solution A has pH of 4.6 and solution B has a pH of 8.0 1- What is the (H3O+) in solution A? 2- What is the (OH-) in solution B ? Thursday, June 3, 2010 at 8:56pm by Lynne
chemistry need help figure out how to do these problem: 1)Calculate the pH of this solution: 1.55 X 10^-2 M HBr 2)Determine the pH of this solution: pOH = 8.3 thanks Tuesday, November 30, 2010 at 11:10am by amy
chemistry A 0.20 M sodium chlorobenzoate (NaC7H4ClO2) solution has a pH of 8.65. Calculate the pH of a 0.19 M chlorobenzoic acid (HC7H4ClO2) solution. Sunday, November 28, 2010 at 9:47pm by justin
Help Chemistry Can you please tell me if these are right? Determine the pH for the following solutions A [OH-] = 1.0 X 10^-7 M I got 7 B. [H3O+ = 4.2 X 10 ^-3M I got 2.4 C. [H3O+]= 0.0001M I got 4 D. [OH-] = 8.5 X10^-9M I got 5.9 What are the [H3O+] and [OH-] for a solution with the followin... Tuesday, December 7, 2010 at 11:01am by Jessica
Chemistry How many moles of NaOH must be added to 1.0 L of 1.4 M HC2H3O2 to produce a solution buffered at each pH? (a) pH = pKa mol (b) pH = 3.07 mol (c) pH = 5.15 mol Sunday, December 5, 2010 at 3:22pm by justin
science a solution of hcl of concentration 1.5 mole/liter is mixed with another solution of hbr of the same concentration. calculate: 1)ph of hcl solution alone 2)ph of the final mixture Sunday, December 12, 2010 at 1:54pm by Mero
chemistry The concentration of HNO3 in a solution is 3.50 10-6 M. What is the [H3O+] in the solution? _______M What is the [OH-] in the solution? ________ M What is the pH of the solution? What is the pOH of the solution? Tuesday, December 21, 2010 at 8:26pm by jim
chemistry Hi, The problem is: "Calculate the concentration of OH- and the pH value of an aqueous solution in which [H30+] is 0.014M at 25C. Is this solution acidic, basic, or neutral?" I have calculated the OH- concentration to be: 7.1 X 10^-14 When I calculate the pH (using H... Wednesday, March 30, 2011 at 2:54pm by LaurenM
chemistry The concentration of NaOH in a solution is 7.00 10-6 M. What is the [H3O+] in the solution? _______________M What is the [OH-] in the solution? __________M What is the pH of the solution? What is the pOH of the solution? HELPP?? i don't understand any of this... Wednesday, December 22, 2010 at 4:17pm by jim
Please Help CHEM Can you please tell me if these are right? Determine the pH for the following solutions A [OH-] = 1.0 X 10^-7 M I got 7 B. [H3O+ = 4.2 X 10 ^-3M I got 2.4 C. [H3O+]= 0.0001M I got 4 D. [OH-] = 8.5 X10^-9M I got 5.9 What are the [H3O+] and [OH-] for a solution with the followin... Tuesday, December 7, 2010 at 2:03pm by Jessica
Chemistry Calculate the end point pH, when 25 mL of 0.01 mol/L HCl solution reacts exactly with 25 mL of 0.1 mol/L NH4OH solution. NH3 Kb = 1.8 x 10^-5 This will be the pH of NH4Cl solution. NH4+ + HOH ==> NH3 + H3O^+ Ka = Kw/Kb = (NH3)(H3O^+)/(NH4^+). Solve for H3O^+, then pH = ... Thursday, May 31, 2007 at 9:02pm by Raj
chemistry Captain Kirk, of the Starship Enterprise, has been told by his superiors that only a chemist can be trusted with the combination to the safe containing the dilithium crystals that power the ship. The combination is the pH of Solution A described below, followed by the pH of So... Tuesday, May 27, 2008 at 9:36pm by Tom
High School Chemistry 10mL of 0.10M HCl is given. What is the pH? How many milliliters of 0.10M NaOH would be required to neutralize it? What is the pH of the neutralized solution? What would the pH of the solution be if you added 20mL of NaOH? Here's what I have so far: pH of HCl=-log(0.10M)= ... Monday, March 21, 2011 at 12:58am by Becky
Chemistry! HB, pH=1 To neutralize 10cm3 it took 5.00cm3 NaOH 10cm3 of the solution HB are diluted with water to make 1 litre of solution. The pH of the new solution is 3. Show that HB is the strongest acid. Tuesday, November 24, 2009 at 5:53pm by Anonymous
chemistry HB, pH=1 To neutralize 10cm3 it took 5.00cm3 NaOH 10cm3 of the solution HB are diluted with water to make 1 litre of solution. The pH of the new solution is 3. Show that HB is the strongest acid. Tuesday, November 24, 2009 at 2:29pm by Anonymous
AP Chemistry A buffer solution contains .4mol of formic acid, HCOOH and a .6mol of sodium formate, HCOONa, in 1L of solution. Ka of formic acid is 1.8 x 10^-4. a) calculate pH b) if 100ml of this buffer solution is diluted to a volume of 1L with pure water, the pH does not change. Discuss ... Sunday, April 25, 2010 at 12:24pm by Jessie
Chem. Can you also check this one, Please and thank-you! 23. Acetylsalicylic acid, commonly known as ASA, is the most widely used drug in the world. ASA has the chemical formula, C8H7O2COOH, and a Ka of 3.27 X 10 – 4 mol/L. What is the pH of a 10 mol/L ASA solution? The pH of t... Wednesday, July 19, 2006 at 11:07pm by Jacy
9th grade science Here are some sites to try about the pH solution: http://search.yahoo.com/search?fr=mcafee&p=If+the+solution+is+known+to+be+0.000+001+M%2C+what+is+the+pH+solution%3F+ Sra Friday, March 11, 2011 at 9:14am by SraJMcGin
chemistry pH = -log(H^+). Plug in 3.00 for pH and calculate (H^+). Since the solution is diluted by a factor of two, then (H^+) in the diluted solution will be 1/2 of the initial value. Plug in the new (H^+) and solve for the new pH. Hint: it will NOT be 1/2 of 3.00. Tuesday, May 5, 2009 at 11:06pm by DrBob222
chemistry The pH of a solution is 6.0. Explain how the addition of the following substance would alter (or not alter) the pH of the solution. a. HCl b. NaOH c. H20 Monday, January 24, 2011 at 10:58pm by steven
Chemistry 1- Determine the [OH-] and pH of a solution that is .250 M in HCO-3 2- Calculate the [H3O+] and pH of each polyprotic acid solution: a) .125 M H2CO3 b) .125 M H3C6H5O7 Monday, March 14, 2011 at 4:56pm by Joey
AP Chem A 0.23 M sodium chlorobenzoate (NaC7H4ClO2) solution has a pH of 8.68. Calculate the pH of a 0.23 M chlorobenzoic acid (HC7H4ClO2) solution Sunday, February 15, 2009 at 11:54pm by Jake
chemistry explain why you get two different pH values for same solution when calculating and using pH meter of same solution? Friday, February 11, 2011 at 9:50am by kabelo
Chemistry I did an experiment on Buffers: In a polystyrene beaker, mix 20 ml of 0.1M Acetic acid ad 25 ml of 0.1 M sodium acetate and immediately measure the pH. Remove the electrode and add 5 ml of 0.1 M HCL to this buffer. Stir the solution and measure the pH. This is my data: Conc.of... Thursday, July 16, 2009 at 3:36am by Saira
Chemistry I have a test on monday and I NEED to ace it in order to raise my grade > . < ldsfkjaslkf right now, acids and bases are killing me can somebody help me with these problems? A buffer solution is prepared by mixing the weak base ammonia (Kb=1.77x10^-5) with ammoni... Saturday, May 15, 2010 at 2:10pm by Kimberlee
Chemistry, Buffers, pH Hi could someone please help me in the next 5 minutes with this question: Given this data: mass of unknown acid 1.4671g Volume of NaOH used in titration 18.47mL Concentration of the NaOH used 0.2403M pH of the original acid solution 2.16 pH of the final acid solution 3.49 Show... Friday, September 26, 2008 at 1:30am by janet
chemistry I asked this before, but got no response. A) If you make up a solution of 250 mL of 0.1 M TRIS in the acid form, what will be the pH? B) If you add 2 mL of 1 M NaOH to the solution in part A, what will be the pH? Thanks. Sunday, February 3, 2008 at 2:43pm by student
chemistry A) If you make up a solution of 50 mL of 0.1 M TRIS in the acid form, what will be the pH? (pka of TRIS: 8.3, molecular wt: 121.1 g) B) if you add 2mL of 1 M NaOH to the solution, what will be the pH? Thank you. Saturday, February 2, 2008 at 4:09pm by matt
Chemistry A solution of acetic acid having a concentration of about 0.2M is to be titrated using 0.200M NaOH. Select an indicator for the titration. what salt will the solution contain at the equivalence point? what is the approximate concentration of this salt at the equivalence point?... Saturday, May 15, 2010 at 2:00pm by Alison
CHEMISTRY/ A student takes a 1.00 mL aliquout of 5.00*10^-4 M HCl solution and dilutes it to the mark with water in a 1000.0 mL volumetric flask. (a)What is the expected pH for the final solution at 25C? (b)What would be the expected pH if this solution were later used at a temperature o... Sunday, March 20, 2011 at 5:38am by TORI
chemistry Water in contact with air is acidic due to the dissolved carbon dioxide. Water in equilibrium with the air contains 4.4 x 10^-6% CO2. The resulting carbonic acid, H2CO3,gives the solution a hydrogen ion concentration of 2.0 x 10^-6M, about 20 times larger than that of pure wat... Saturday, March 24, 2007 at 1:06pm by Heather
chemistry after finding the ph of the corresponding ions in these two questions, would you add the two ph's together to determine the final ph of the solution? Saturday, April 18, 2009 at 3:05pm by Anonymous
chemistry Find the pH of a 0.010M solution of NH4ClO4 and the pH of a 0.010M solution of NH4C2H3O2. Saturday, April 18, 2009 at 3:05pm by Hannah
chemistry Adding acid will make it more acid; pH will go down. Adding base will make the solution more basic; pH will go up. Adding water will make the solution more dilute and it will change the pH somewhat (a little more basic making pH go up); how much depends upon how much water is ... Monday, January 24, 2011 at 10:58pm by DrBob222
chemistry The pH at the beginning of the titration is just the pH of a 0.2 M HF solution. b). moles HF = M x L = ?? moles NaOH = M x L = ?? Which is in excess. Subtract. If HF in in excess, you will have a buffer solution of HF and NaF. If NaOH is in excess the pH will be determined by ... Saturday, November 6, 2010 at 5:04pm by DrBob222
chemistry lab Could someone help me with this? i am tired of it. here is my data from lab: Buffer1: HPO4- weight 3.412g; original pH Buffer 2: HEPES wt: 1.090g original pH 10.08 buffer1: pH of 0.1M: 7.5; pH of 0.01: 7.72; pH of 0.001M: 7.87 buffer2: PH of 0.1M: 7.5 ph of 0.01 M: 7.42 pH of ... Friday, February 1, 2008 at 10:54pm by amanda
chem I don't think so. Now that I see the question again, I'm wondering if this is a problem with two parts; i.e., the question is asking for the pH of 0.0515 M HCl and for the pH of a separate solution of 0.0762 M NaC2H3O2? And after noticing that there is no volumes liste... Thursday, April 16, 2009 at 2:09pm by DrBob222
Chemistry Use solution B to solve for the Ka of the weak acid. Use Ka from above to solve for the pH of solution A. That gives you the first 3 numbers of the combination. Use solution C and the Henderson-Hasselbalch equation to solve for the pH of that solution which will be last three ... Tuesday, May 27, 2008 at 7:38pm by DrBob222
Chemistry NH3 + HCl ==> NH4Cl moles NH3 = M x L = ?? moles HCl = M x L = ?? Determine from the moles you have which reagent is in excess, determine the molarity from M = mole/L and find pH of the resulting solution. I suspect NH3 is in excess and that will produce a buffered solu... Sunday, February 13, 2011 at 11:32pm by DrBob222
Pre Calculs The pH of a chemical solution is given by the formula pH = -log10 [H+] where [H+] is the concentration of hydrogen ions in moles per liter. Values of pH range from 0 (acidic) to 14 (alkaline). (a) what is the pH of the solution for which [H+] is 0.1? (b) What happens to pH as ... Tuesday, October 10, 2006 at 1:06pm by Erica
chemistry What is th pH of a buffer solution made by dissolving 0.10 mol of formic acid, HCOOH, and 0.10 mol of sodium formate, HCOONa, in 1L of water? What is the molarity of a solution made by dissolving 3.4g of Ba(OH)2 in enough water to make 450mL of solution? Assume that Ba(OH)2 io... Wednesday, November 18, 2009 at 9:53pm by Taylor
science What is the [Pb+2] in a saturated solution of Pb(OH)2 for each of the following initial pH values? Ksp Pb(OH)2 = 2.8x10-16 a. pH = 13.00 b. pH = 9.20 Monday, January 31, 2011 at 11:48am by N/A
chemistry SALT HYDROLYSIS 1.) Calculate the pH of a 0.24M sodium formate (HCOONa) solution. Kb=5.9x10^-11. 2.) Calculate the pH of 0.25M pyridium chloride (C5H5NHCl)solution. Ka=5.9x10^6. Thursday, January 20, 2011 at 5:18am by jaycab
science Assume that you have a pH meter which would enable you to very accurately measure the pH of a solution. Describe an experimental design that would allow you to pinpoint the exact pH at which Catalase is the most active. Friday, March 11, 2011 at 9:35am by anonymous
chemistry In a buffer solution, if [Aƒ{] < [HA], which of the following must be true? a. pH < pKa b. pH = pKa c. pH > pKa d. pH < 7.00 e. pH > 7.00 Wednesday, November 10, 2010 at 4:13pm by miller
Chemistry IN the polystyrene beaker, mix 20mL of 0.1 M Acetic acid and 25mL of 0.1M Sodium Acetate and immediately measure the pH. Remove the electrode and add 5ml of 0.1 M HCl to this buffer. Stir the solution and measure the pH. _______________ INFO: concentration of acetic acid= 0.1M... Sunday, March 28, 2010 at 5:53pm by Saira
Chemistry/pH- Weak Acid Hi again! I have a new question, Can you help me? Consider 50.0 mL of a solution of a weak acid HA (Ka = 1.00.E-6), which has a pH of 4.000. What volume of water must be added to make the pH = 5.000? My Calculations: To calculate the concentration of x, I take the pH value -&a... Sunday, August 17, 2008 at 6:07am by Mary
chemistry Aqueous solution with a pH of 10.6 is diluted from 1 L to 1.5 L. What is the pH of the diluted solution? Sunday, March 14, 2010 at 6:39pm by elizabeth
chemistry An aqueous solution with a pH of 3.00 is diluted from 2.0 L to 4.0 L. Wht is the pH of the diluted solution? Tuesday, May 5, 2009 at 11:06pm by j
chem class What is the pH of an aqueous solution at 25.0 °C that contains 3.98 × 10-9 M hydroxide ion? i posted this before and i tried solving it but i get it wrong 14 = ph + - log (3.98 × 10-9) 14- 8.4 = ph 5.6 = ph but the correct answer is 8.400 what did i do wrong? Sunday, November 21, 2010 at 7:51pm by jessie
chemistry a 5.55g sample of a weak acid with ka=1.3*10^-4 was combined with 5.00ml of 6.00 M NAOH and the resulting solution was diluted to 750mL. The measured pH of the solution was 4.25. what is the molor mass of the weak acid. if used the formula pH=kpa+log(base/acid) Ph=3.89+log(6.0... Thursday, November 25, 2010 at 1:55pm by help
chemistry a 5.55g sample of a weak acid with ka=1.3*10^-4 was combined with 5.00ml of 6.00 M NAOH and the resulting solution was diluted to 750mL. The measured pH of the solution was 4.25. what is the molor mass of the weak acid. if used the formula pH=kpa+log(base/acid) Ph=3.89+log(6.0... Thursday, November 25, 2010 at 1:52pm by help
chemistry what is the pH of a solution that is .15 M in HOCl and .25 M NaOCl after .05 mol HCl/L has been bubbled into the solution? this is what I did: HOCl + H2O ----> H3O+ + OCl- .15 .25 -.05 +.05 --------------------------- .1 .30 3.5E-8=[H3O][.3]/[.1] H3O= 1.167E-8 pH= -log(... Tuesday, November 23, 2010 at 11:44am by Audrey
Chemistry I figured out the correct new pH for each respective part, but apparently the initial pH i found for the buffer solution is incorrect. I just need help in figuring that so I can calculate the change. I initially thought the buffer pH was 7.38. Thanks! Tuesday, March 16, 2010 at 11:52pm by Trixie
chemistry When a strong acid is added (exactly neutralized) to a strong base, the salt produced is neutral (neither cation nor anion is hydrolyzed) and the pH = 8. When a weak acid and a salt of the weak acid are present in solution, you hve a buffered solution and you must use the Hend... Sunday, July 11, 2010 at 11:12pm by DrBob222
chemistry-science A 500 ml buffer solution contains .2M Acetic acid and .3M sodium acetate. Find the pH of the buffer solution after adding 20 ml of 1M NaOH, what is the pH? (pka = 4.74) Friday, April 30, 2010 at 3:22am by jess
Chemistry What will be the pH of: (a)10.0cm3 of an aqueous solution of 0.001mol dm^-3 nitric aicd, HNO3 (aq)? (b)100cm3 of an aqueous solution of 0.001mol dm^-3 nitric aicd, HNO3 (aq)? (c)0.02mol dm^-3 of potassium hydroxide solution, KOH (aq)? For (a) I got 2, (b) 1 and (c) 12.31. I am... Tuesday, November 17, 2009 at 3:47pm by Anonymous
Chem Consider a solution that contains both C5H5N and C5H5NHNO3. (Kb for pyridine, C5H5N, is 4.0 x 10^-4) (a) Calculate the ratio of [C5H5N]/[C5H5NH+] if the solution has a pH of 4.50. (b) Calculate the ratio of [C5H5N]/[C5H5NH+] if the solution has a pH of 5.00. Tuesday, April 7, 2009 at 12:36am by Fred
CHEMISTRY--URGENT HNO3 with pH 3 is mixed with 2 L KOH with pH 12. assuming volumes are additive what is the pH of the final solution? I have absolutely no idea how to do this. I do know the answer, though. I have a test tomorrow and I would really appreciate it if someone could help!!!! Sunday, May 2, 2010 at 11:59pm by Maggie
chemistry Will this solution form a buffer? 100 mL of .10 M NH3; 100 mL of .15 M NH4Cl Work: NH3= .01 moles NH4Cl= .015 moles .... not sure what else to do. I think we use the H-H equation, but I don't know how to find pKa, or even what pKa is. This should give the pH of the solutio... Friday, March 19, 2010 at 7:41pm by Vanessa
Chemistry II If 15.0 mL of 1.2e-4 mol/L HI is added to 26.0 mL of 9.2e-4 mol/L HI, what is the pH of the solution? M x L = mols. Calculate mols for solution 1, do the same for solution 2, add mols together and divide by total liters. That will be the new molarity. Then pH = -log(Molarity) Tuesday, April 24, 2007 at 9:39pm by Jayd
Chemistry If 100mL of a 0.10M NaOH solution is added to 75mL of a 0.15 HCl solution, then what is the pH of the resultant solution? Wednesday, August 22, 2007 at 10:10pm by Bert
biology If the pH of a sample was 3 how many times more acidic is it than a solution with a pH of 6? Sunday, November 2, 2008 at 8:13pm by Astrid
Chemistry The pH of a NaHCO3 solution is independent of the concn. pH = 1/2(pk1 + pk2) Tuesday, April 13, 2010 at 9:51pm by DrBob222
Gen CHEM 2 This is all they gave me: You need to produce a buffer solution that has pH 5.28. You already have a solution that contains 10 millimoles of acetic acid. How many millimoles of solid sodium acetate will you need to add to this solution? The of acetic acid is 4.74. Then they ga... Monday, February 11, 2008 at 9:42pm by Jessica
chemistry predict the pH of the solution obtained when a 1.0 M magnesium hydroxide solution is titrated with an equal amount of a 1.0 M solution of sodium chloride. Monday, March 29, 2010 at 5:45pm by Ash
chemistry a saturated solution of milk of magnesia, Mg(OH)2, has a pH of 10.5. What is the hydronium concentration of the solution? is the solution acidic or basic? Tuesday, July 14, 2009 at 7:10pm by angela
Chemistry/pH- Weak Acid Hi again! I have a new question, Can you help me? Consider 50.0 mL of a solution of a weak acid HA (Ka = 1.00.E-6), which has a pH of 4.000. What volume of water must be added to make the pH = 5.000? My Calculations: To calculate the concentration of x, I take the pH value -&a... Sunday, August 17, 2008 at 6:01am by Mary
College Chemistry Calculate both [H30] and [OH-] for a solution that is: pH=5.50 ph=7.00 Sunday, April 26, 2009 at 10:15pm by Gayla
Chemistry What is the pH of a buffer solution that is 0.20M methylamine and 0.15 M methylammonium chloride. which do i get the pH of Wednesday, April 2, 2008 at 12:09am by LT
Chemistry .12M Lactic Acid (HC3H5O3, Ka=1.4x10^-4) is mixed with .10M NaC3H5O3 to form 1.00L solution. A. Calculate the pH of the solution after the addition of 50.0mL of 1.00M NaOH. B. Calculate the pH of the solution after the addition of 120.0mL of 1.00M NaOH. Sunday, March 28, 2010 at 12:16pm by Emma
chemistry NH3 + HCl ==> NH4Cl So you have 8 x 10^-4 moles each. That means the solution is exactly neutralized; therefore, the pH of the solution will be determined by the hydrolysis of NH4Cl. Write the hydrolysis equation for NH4^+, set up an ICE chart, and solve for H3O^+, then... Saturday, April 24, 2010 at 11:15pm by DrBob222
Survey of the sciences When the hydronium ion comcentration of a solution equals 1 mole per liter, what is the pH of the solution? Is the solution acidic or basic? Wednesday, February 9, 2011 at 5:12pm by Stephanie
chemistry A buffered solution is made by adding 50.0 g NH4Cl to 1.00 L of a 0.84 M solution of NH3. Calculate the pH of the final solution Tuesday, August 10, 2010 at 3:14pm by chris
Chemistry Acid/bases The concentration of H2SO4 in a solution is 3.20 10-6 M. Assume the acid dissociates completely in solution. What is the [H3O+] in the solution? What is the [OH-] in the solution? What is the pH of the solution? What is the pOH of the solution? OK SO I KNOW HOW TO DO THESE TYP... Tuesday, February 10, 2009 at 8:11pm by Spencer
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