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April 20, 2014

Search: Calculate the pH of a 0.21 M CoCl3 solution. The Ka value for Co(H2O)63+ is 1.0 10-5.

Number of results: 27,869

chemistry
How to calculate PH 1.9 = 0.0126M Why? How to calculate PH 1.8 = ? How to calculate PH 20 = ? How to calculate PH 21 = ? Pls helps me
Sunday, August 5, 2012 at 1:09pm by Fai

Chemistry
Calculate the pH of a 100mL solution of 0.10M acetic acid ka=1.8x10(-5) i calculated the pH to be 2.87 from the square root of (1.8x10(-5) * 0.1, the negative log gives me the pH. The next question wants you to calculate the pH with 50mL HCl added. I found the pH to be 2.78 by...
Tuesday, October 25, 2011 at 12:38am by Kevin

chemistry
Calculate the pH range required to separate 99.99% of Cr3+ from Zn2+ by precipitation of Cr(OH)3(s) in a solution that is initially 0.034 M in both Cr3+ and Zn2+. Use the Ksp values from Table 16.2 of Chang and calculate the pH to the nearest 0.01 pH unit. Lowest pH= Highest pH=
Sunday, March 25, 2012 at 5:17pm by Tanner

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 H30+), I ...
Wednesday, March 30, 2011 at 2:54pm by LaurenM

chemistry
Is this all of the information you have? I think you need the pH at SOME point, or a way to calculate pH at the beginning or the end and I don't see a way to do it without other information. The usual way is to calculate moles of the acid (moles = grams/molar mass) and use ...
Monday, November 22, 2010 at 12:32am by DrBob222

chemistry
how to calculate PH =1.9 therefore =0.0126M I do not understand only this part about PH = 0.0126M Please tells me how to calculate the PH = 1.9 = 0.0126M Other way to calculate 0.0126Moles = PH 1.9 0.0126M x 4.85L=0.061mole 0.061mole x 36.46 = 2.22g 2.22g /0.36 = 6.16 6.16/1....
Saturday, August 4, 2012 at 10:31pm by Fai

Chemistry
Calculate the molar hydroxide ion concentration of each of the following solutions given the pH: pH=0.90 AND pH=1.62 I know to covert from ph to hydroxide but i'm having a problem going from hydroxide to ph..can someone please help me..thanks
Thursday, May 5, 2011 at 12:38pm by Renee

chemistry
a. neither Na^+ nor Cl^- are hydrolyzed; therefore, the pH is just that of pure H2O which is pH = 7. b. KCN the CN^- is hydrolyzed. CN^- + HOH ==> HCN + OH^- so you know it will be basic. You can calculate the actual pH but that isn't necessary. c. LiF the F^- is hydrolyzed...
Tuesday, March 26, 2013 at 11:04pm by DrBob222

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
Calculate it to see. pH = 4 so (H^+) = 1 x 10^-4 M (use pH = -log(H^+) to calculate that). Then use mL x M = mL x M to calculate the new pH.
Sunday, April 25, 2010 at 1:24pm by DrBob222

chem
Consider the titration of 20 mL of .105M Butric Acid HBut, with .125M sodium Hydroxide? calculate the pH before titration calculate the volume of added base to reach the end point calculate the pH halfway to the equivalence point kb(But-)= 6.6x 10^-10 and ka(HBut)= 1.5x 10^-5 ...
Monday, March 1, 2010 at 11:38pm by simi

Chemistry
If the problem is to calculate the pH of the buffer, then you must have the concn of NH4NO3. Or if you were given a pH of the buffer, you can calculate the concn of NH4NO3 needed to produce that pH. You must know one of them to calculate the other.
Friday, November 11, 2011 at 8:45pm by DrBob222

Chemistry
I guess I am still stuck on problem a. I know I have to calculate Ka from Kb in order to calculate pH. When I do that, I get a pH over 14 which cannot be. What am I doing wrong?
Monday, April 1, 2013 at 8:36pm by Jill

Chemistry
I guess I am still stuck on problem a. I know I have to calculate Ka from Kb in order to calculate pH. When I do that, I get a pH over 14 which cannot be. What am I doing wrong?
Monday, April 1, 2013 at 8:36pm by Jill

chemistry
for a .001M solution of methionine: a) calculate the isoelectric pH b) calculate the isoionic pH
Sunday, April 7, 2013 at 7:58pm by Lana

chemistry
calculate the Ph of 0.3 M sodium propanoate, Ka 2.0 x 10 base -3. then calculate the pH after 0.03 mol NCL is added to 2L of the first solution.
Saturday, July 20, 2013 at 1:36pm by Mandy

chemistry
Calculate the solubility of Mn(OH)2 in grams per liter when buffered at each of the following. (a) pH 7.7 (b) pH 9.6 (c) pH 11.3
Wednesday, March 27, 2013 at 10:35am by hannah

chemistry - quant.
I need help calculating the pH of a solution that is .0400M Na3AsO4 I was trying to calculate the pH with [H30+]=sqrt(ka1*ka2) What is the correct way to calculate this? Thankyou
Thursday, December 13, 2007 at 12:28pm by anon

AP CHEMISTRY
Calculate the solubility of Mn(OH)2 in GRAMS PER LITER when buffered at each of the following. a)pH 7.4 b)pH 9.2 c) pH 11.5
Saturday, March 10, 2012 at 4:01pm by JIM

AP CHEMISTRY
Calculate the solubility of Mn(OH)2 in GRAMS PER LITER when buffered at each of the following. a)pH 7.4 b)pH 9.2 c) pH 11.5
Saturday, March 10, 2012 at 4:14pm by fernatesfsdf

chemistry
millimols HCl = 35 mL x 0.342M = ? mmols NaOH = 5 x 0.173 = ? Calculate each, determine the one in excess, calculate the amount in excess, then if acid pH = -log(H^+) or if basic then pOH = -log(OH^-) and convert to pH by pH + pOH = pKw = 14.
Wednesday, December 5, 2012 at 11:30am by DrBob222

Chemistry
A titration is performed by adding .600 M KOH to 40.0 mL of .800 M HCl. Calculate the pH before addition of any KOH. Calculate the pH after the addition of 5.0 mL of the base. Calculate the volume of base needed to reach the equivalence point. What is the pH at the equivalence...
Friday, April 1, 2011 at 1:18pm by Summer

Chemistry
Consider a solution that contains both C6H5NH2 and C6H5NH3+. Calculate the ratio [C6H5NH2]/[C6H5NH3+] if the solution has the following pH values. (Assume that the solution is at 25°C.) (a) pH = 4.70 (b) pH = 5.26 (c) pH = 5.42 (d) pH = 4.96
Wednesday, March 13, 2013 at 2:47am by Margaret

Chemistry
Calculate the molar hydroxide ion concentration of each of the following solutions given the pH: pH=0.90 AND pH=1.62 I know to covert from ph to hydroxide but i'm having a problem going from hydroxide to ph..can someone please help me..thanks can someone please answer my ...
Thursday, May 5, 2011 at 12:38pm by Renee

chemistry
acetic acid: 0.1 M 30ml hydrochloric acid 0.1 M 5 ml sodium hydroxide 0.1 M 15 ml Buffer + 5ml of: 1.91 ph ph (measured): 4:52 ph HOW DO I CALCULATE PH(CALCULATED)? AND ALSO IT SAYS SHOW YOUR CALCULATION FOR THE PH OF THE BUFFER BEFIRE AND AFTER THE ADDITION OF HCL? COULD YOU ...
Saturday, July 14, 2012 at 6:28pm by fenerbahce

chem
a buffer is made by adding 150 ml of .595M BaF2 and 0f .500M of HF solution. calculate the pH of this buffer system calculate the pH of this buffer after adding .100 mol Hcl calculate the pH of this buffer after adding .0750 mol Ca(OH)2 ka(HF)= 6.9x10^-4 kb(F-)= 1.4 x 10^-11
Monday, March 1, 2010 at 11:37pm by simi

Chemistry
Neither K^+ nor Cl^- are hydrolyzed; therefore, the pH is just that of H2O. (H^+)(OH^-) = Kw = 1E-14. Solve for H^+ and convert to pH. pH = 7.00. Note: I assume this is a lower level course; if not that you must calculate the ionic strength of the 1.7M KCl solution and the pH ...
Wednesday, July 4, 2012 at 1:19pm by DrBob222

Chemistry - pH
Calculate the pH of each of the following solutions: a) .35 M hydrochloric acid, HCl b) .35 M acetic acid, HC2H3O2 c) .35 M sodium hydroxide, NaOH Can someone please explain to me how to calculate the pH in a way that is easy to understand? I am confused. Could you please do ...
Monday, September 14, 2009 at 10:12am by Mandy

Chemistry
I suspect the problem is that the question asks for CHANGE in pH and you're giving the data base the pH. I think something like 1.128 which I would round to 1.13 is the answer for the HCl part. I didn't work the NaOH part. pH = pKa + log(9.24/0.7). pH = pKa + 1.128. I didn't ...
Tuesday, March 27, 2012 at 6:01pm by DrBob222

Chemistry
Calculate the pH of a 50.0 mL solution 0.0120 M ethylaminium chloride (C2H5NH3Cl ) and 0.0360 M ethylamine C2H5NH2. Kb = 4.3 x 10-4 Calculate the pH when 5.0 mL of 0.1 M HI is added. Ignore any changes in the volume
Wednesday, April 17, 2013 at 12:54am by m

Chemistry
Calculate the pH of a water sample from a playa lake in the western US that has the evaporite mineral potassium bicarbonate (KHCO3) at a concentration of 0.009 mol/kg. Assume the water is in equilibrium with the atmosphere (PCO2 = 10-3.4 bar) and the temperature is 25 ̊C...
Sunday, February 10, 2013 at 11:49pm by Ashley

Chemistry
Calculate the pH of a 5.90 10-3 M solution of H2SO4 I have tried doing this as pH=-log[H+] and also by multiplying the Molarity by two because there are two hydrogens and then doing the -log but both ways have gotten me the wrong answer is there something i am missing? same ...
Monday, March 5, 2012 at 9:54pm by Ashley

chemistry
The only way I know to do this is to calculate the buffer capacity of each, then compare them. The buffer capacity is the number of moles of a strong acid or a strong base that causes 1.00 L of the buffer to undergo a 1.00 unit change in pH. So you calculate the pH of the ...
Sunday, December 12, 2010 at 5:28pm by DrBob222

Chemistry
Calculate pH from the Henderson-Hasselbalch equation to give you the initial pH. Then to that buffer you add 2.50 mL x 0.150 M HCl to 100 mL. That will add 0.000375 moles HCl. That will increase the mole CH3COOH by that amount and decrease moles CH3COONa by that amount. ...
Sunday, April 11, 2010 at 11:44pm by DrBob222

chemistry
a)Calculate the pH of a solution of 0.75 M HNO3, which is a strong acid. b)Calculate the pH of a 1.0 L aqueous solution made from 0.80 mol CH3COOH and 0.20 mol KCH3COO (Ka = 1.8 x 10^-5).
Thursday, May 9, 2013 at 9:36am by alex

Chemistry
HBr + KOH ==> KBr + HOH moles HBr initially = L x M = ? moles KOH added = L x M = ? See which is in excess and calculate pH from pH = -log (H^+). OR if mole HBr = moles KOH, the the solution has just KBr and H2O and calculate pH from that. Post your work if you need ...
Thursday, July 16, 2009 at 4:35pm by DrBob222

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

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 -&...
Sunday, August 17, 2008 at 6:07am by Mary

Chemistry
Can someone please help me here? It's review for my test. Thanks! Calculate the expected pH of the buffer prepared in Part I of this lab. The Ka of acetic acid is 1.8 x 10-5 Calculate the expected pH when 10.0mL of 0.10M HCl is added to the buffer from question 3 Calculate the...
Tuesday, April 8, 2014 at 9:54am by Matt

chemistry
Now take another 35 mL of the 0.50 M pH 6.59 buffer and add 1.5 mL of 1.00 M NaOH. Using steps similar to those above, calculate the new pH of the solution. find pH
Monday, October 24, 2011 at 2:53pm by Taylor

Chemistry
How do you calculate the following: Starting with a liter of 1M sodium acetate (pka of acetic acid = 4.75 ), calculate the number of moles of strong acid or strong base needed to make a pH buffer effective at pH = 4.o ? Thank you!
Wednesday, June 29, 2011 at 8:19pm by Maria

chemistry
Who told you the correct answer is 7.00? That isn't right. Reason through it. Low pH means high pOH (since pH + pOH = 14) and that means high H^+. So for high OH^- we want a high pH which means a low pOH and that is a high OH^-. If you don't like that method, go through and ...
Saturday, December 11, 2010 at 1:07pm by DrBob222

Chemistry/pH- Weak Acid
For a pH = 4, [H+] = antilog(-4.000) = 1.00x10^-4 Ka = [H+][A-] / [HA] Let [H+] = [A-] = x Ka = x^2 / (c - x) , where c = molar concentration of HA before dissociation. if c is much larger than x, we can simplify the expression to: Ka = x^2 / c (1.00x10^-6)c = 1.00x10^-8 c = 1...
Sunday, August 17, 2008 at 6:01am by GK

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 2
A titration is performed by adding 0.124 M KOH to 40 mL of 0.159 M HNO3. a) Calculate the pH before addition of any KOH. b) Calculate the pH after the addition of 10.26, 25.65 and 50.29 mL of the base.(Show your work in detail for one of the volumes.) c) Calculate the volume ...
Tuesday, April 2, 2013 at 10:44pm by Antonio

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 to ...
Wednesday, April 29, 2009 at 8:23pm by DrBob222

Chemistry, pH, Buffers
Please help!! 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 me how do I calculate the Ka of the unknown acid and the ...
Monday, April 2, 2012 at 11:44am by Krina

chemistry
HC2H3O2 ==> H^+ + C2H3O2^- Ka = (H^+)(C2H3O2^-)/(HC2H3O2) Calculate (H^+) from pH = -log(H^+). Calculate (C2H3O2^-) from g of the trihydrate. That is moles = grams/molar mass and mole/L (L is 0.15) = M Calculate (HC2H3O2) from L x M = ? Plug in and calculate Ka. For part 2...
Thursday, July 16, 2009 at 7:35pm by DrBob222

Chemistry
Calculate the amount of H2SO4 needed to make 1.00L of acid rain with a PH equal to the average PH of rain in Maine (ph = 5.0). Concentration of H2SO4 to use = .00100M I am absolutely confused...please help
Wednesday, January 23, 2013 at 6:24pm by Henry

biochemistry
A weak base has pKb = 9.25.. A. Calculate the % ionization at pH = 8.25 B. Calculate the % ionization at pH = 10.25 C. What is the pH when 50% of the weak base is ionized?. Is calculating ionization for pkb the same as pka? How do I go about doing it?
Tuesday, August 24, 2010 at 6:10pm by elizabeth

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 -&...
Sunday, August 17, 2008 at 6:01am by Mary

Chemistry
pH = -log(H^+) Plug in 6 for pH and calculate (H^+). Then remember that pH + pOH = 14 and do OH^- the same way (except plug in 8 for pOH).
Tuesday, August 28, 2007 at 9:22pm by DrBob222

Chemistry
1.CALCULATE pH of 1.0 L 0.010 M ascetic acid and 0.50 L 0.010 M NaOH. 2. Calculate pH of 1.0 L 0.010 M NaOH and 0.500 L 0.010M HCl Buffer help?
Thursday, March 15, 2012 at 8:58pm by ALISON

ap chem
A 9.00 M solution of a weak acid, HA, has a pH of 1.30 1.) calculate [A-] at equilibrium 2.) calculate [HA] at equilibrium Use pH to get (H^+). Ka = (H^+)(A^-)/(HA) (A^-) = (H^+). (HA) = 9 Plug and chug. Post your work if you get stuck.
Thursday, March 22, 2007 at 4:49pm by Jaron

Chemistry
You can use the Henderson-Hasselbalch equation to calculate pH or you can set up the Ka expression and substitute (HBrO) where needed and use (NaBrO) as (BrO^-) in the Ka expression. Calculate H^+ and pH from that.
Tuesday, March 16, 2010 at 7:46pm by DrBob222

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
Chester makes 1L of a 0.01M HCl solution and measure the pH. Burt then adds 5.80 g of sodium chloride to Chester’s solution and measures the pH. Calculate the difference between the two pH values obtained.
Friday, February 14, 2014 at 6:05pm by Anonymous

Chemistry
For the titration of 25.00 mL of 0.150 M HCl with 0.250 M NaoH, calculate (a) the initial pH; (b) the pH when neutralization is 50% complete; (c) the pH when neutralization is 100% complete; and (d) the pH when 1.00 mL of NaOH is added beyond the equivalence point.
Tuesday, August 11, 2009 at 7:25am by ChemHurts

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
Calculate the pH of a solution in which a. [H3O+] = 7.8 x 10-7 M pH = b. [H3O+] = 5.1 x 10-6 M pH = c. [H3O+] = 6.1 x 10-5 M pH = d. [H3O+] = 9.3 x 10-4 M pH = I get 8.1 9.5 9.1 6.7 but its wrong please someone help!
Wednesday, March 19, 2014 at 5:03pm by Danny

science
calculate the pH of pure water. (recall that pH= -log[H+]) Hopefully the following site will help you: http://en.wikipedia.org/wiki/PH
Saturday, December 30, 2006 at 10:11pm by michelle

CHEMISTRY
pH = -log(H^+) pOH = -log(OH^-) pH + pOH = pKw = 14 and (H^+)(OH^-) = Kw. One or more of the four above will calculate all you ever need to know abouat H^+), (OH^-), pH and pOH.
Saturday, May 5, 2012 at 6:01pm by DrBob222

Chem
I think you need the volumes of each although you can assume equal volumes, I think, since both are strong acids. Are you to look up the activities or calculate them from the Debye-Huckel equation or the extended D-H equation. In any event, you will need to calculate the ionic...
Wednesday, November 12, 2008 at 10:50pm by DrBob222

General Chemistry
How do I calculate the ratio of weak base to weak acid in a methyl amine buffer solution at pH=10.645 and pH=11.645 and pH=9.645?
Monday, February 27, 2012 at 8:05pm by Nhi Song

Chemistry
How can I suggest a reason for the deviation for the pH of 4 M HCl? As my answer I put, The pH of 4 M HCl is negative because a molarity of an acid solution greater than 1 produces a negative pH. A negative pH means that the concentration of H+ or H3O+ ions is greater than 1 ...
Wednesday, March 7, 2007 at 12:18pm by Meche

biochemistry
Calculate the pH change of 10mL of HCl added to 1M phosphate buffer in 1L with initil pH of 7.2?
Tuesday, September 28, 2010 at 10:08am by Lina

chemistry
See your post above. The same rules apply here but you are asked to calculate pH. For that, pH = -log(H^+).
Monday, December 5, 2011 at 12:28pm by DrBob222

General Chemistry-Acids/Bases
I'm stuck on a couple of similar problems involving pH and acids/bases 1) What is the final pH of a 1L solution that is initially .15 M HF and .2 M NaF after 10 mL of .02 M HCl has been added? Ka=7.2x10^-4 Do i just calculate the total mols of H and divide by the volume, then ...
Wednesday, November 26, 2008 at 2:18pm by Evelyn

chemistry pH
calculate [H^+] and the pH of 0.025M of HNO3
Saturday, March 9, 2013 at 6:02pm by holly

chemistry
For each titration of a buffer, how do i calculate how many mLs of titrant were required to obtain a 1.00 pH unit change from the initial pH?
Sunday, February 27, 2011 at 4:45pm by Wendy

chemistry
1. Calculate pH of an acetate buffer containing 27.5 mM acetic acid (pKa is 4.74) and 50 mM sodium acetate. When a 30 mM aq solution of sodium acetate was prepared in the lab it had a pH of 8.8. Calculate the amount of acetic acid (in g) to be added to 0.5 L of this sodium ...
Saturday, April 12, 2014 at 1:07pm by Nick

Chemistry
Calculate pH of an acetate buffer containing 27.5 mM acetic acid (pKa is 4.74) and 50 mM sodium acetate. When a 30 mM aq solution of sodium acetate was prepared in the lab it had a pH of 8.8. Calculate the amount of acetic acid (in g) to be added to 0.5 L of this sodium ...
Saturday, April 12, 2014 at 7:31pm by Sarah

Science
Which solution below has the highest concentration of hydronium ions? pH = 9.82 pH = 12.6 pH = 7.93 pH = 3.21 pH = 7.00
Tuesday, March 19, 2013 at 4:25pm by DrewS

Chemistry
Which solution below has the highest concentration of hydronium ions? pH = 9.82 pH = 12.6 pH = 7.93 pH = 3.21 pH = 7.00
Tuesday, March 19, 2013 at 7:26pm by DrewS

chemistry
Calculate the pH of .100 of a buffer solution that is .25 M in HF and .50 M in NaF. What is the change in pH on addition of the following? A. .002 mol of HNO3 B. >004 mol of KOH I calculated the correct pH of the solution but am having trouble calculating A & B. Thanks, Ivy
Saturday, February 1, 2014 at 7:11pm by Ivy

Chemistry
Classify each of the following solutions as acidic, basic, or neutral based on the pH value. (a) pH = 8.0 (b) pH = 7.0 (c) pH = 3.5 (d) pH = 6.1
Saturday, July 30, 2011 at 8:09pm by norma

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

Biochemistry
calculate Ph occuring when 100ml of 0.10m acid is added to 500ml of 0.08m acetate buffer,pka 4.75,ph 4.5
Tuesday, August 2, 2011 at 4:25am by Pearl

Chemistry(Please help)
Calculate the pH of an aqueous solution of 0.15 M potassium carbonate. I know that pH = -log(H30+) but I am not sure how to start this problem.
Saturday, April 14, 2012 at 8:54pm by Hannah

Chem
Calculate the pH of a solution composed of 155mL of 0.1 M acetic acid and 45 g of sodium acetate. The pKa of acetic acid is 4.76. MY ANSWER: pH = 4.76 + log(3.53M/0.1M) pH = 6.31
Tuesday, March 6, 2007 at 9:28pm by Marisol

AP CHEMISTRY
Calculate the solubility of Mn(OH)2 in grams per liter when buffered at each of the following. a) pH 7.4 b) pH 9.2 c) pH 11.5 ALL IN GRAMS PER LITER. PLEASE HELP ME AND EXPLAIN
Monday, March 12, 2012 at 7:21pm by HELP PLEASE

Chemistry
i. calculate the pH of the .833 sodium acetate solution ii. Calculate the pH after adding .700 grams of NaOH to the 35 ml of .833 M sodium acetate solution iii. Calculate the pH after adding 1.5 mL of 12 M HCl to the original 35 mL of .833 M sodium acetate solution
Friday, April 30, 2010 at 8:09am by becca

chemistry
calculate the volume of 3M HCl needed to change the pH of 50 mL of the undiluted buffer solution by one pH unit?
Wednesday, March 16, 2011 at 6:51pm by Anonymous

chemistry
1)A solution has a [OH-] of 5.2 x 10-4. What is the [H3O+] in the solution? 2) A 0.25 M solution of a monoprotic acid, HA, has a pH of 2.54. What is Ka for this acid? The dissociation of HA is: HA + H2O <--> H3O+ + A- (Hint: write the expression for pH) 3 A solution has...
Sunday, December 9, 2012 at 3:17am by nicki

Chemistry
Okay, so based on the chart in my book I was able to determine the following. pH=(unknown) pKa=7.2 of Phosphoric Acid (2) A-=.5M of Na2HPO4 HA=.3M H2PO4- pH= 7.2 + log(.5/.3) pH=7.2+log(1.6667) pH=7.2+0.5108 So, the pH of this solution is: pH=7.7108 Correct?
Wednesday, July 6, 2011 at 11:13am by Shaun

AP CHEMISTRY
a and b are salts. The pH of those solutions is determined by the hydrolysis of the salt. c is a mixture; you calculate the molarity of the acetate ion and go from there. Here is how you do the first one, in detail. .............F + HOH ==> HF + OH^- initial.....0.1...
Thursday, February 16, 2012 at 4:36pm by DrBob222

chemistry
If I have a set of data that gives the apparent partition coefficient as a function of pH, over a range of pH 2-10, how do I calculate the Ka of the compound?
Friday, March 12, 2010 at 3:25pm by Renee

chemistry
If this is not an advance course (in which you need to calculate the ionic strength and use the Debye-Huckel theory), the pH of a KCl solution is simply that of pure water which is pH = 7.0.
Wednesday, July 6, 2011 at 6:28pm by DrBob222

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

Science
a. (H^+)(OH^-) = Kw -= 1E-14 b. X = pH of 5; Y = pH of 4. c. pH = -log(H^+) Solve for (H^+)l. d. pH < 7 = acid pH = 7 = neutral pH > 7 = basic e. See b and d. f. pH + pOH = pKw = 14; then pOH = -log(OH^-)
Monday, September 10, 2012 at 1:03pm by DrBob222

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

Science-Chemistry
Methyl amine is a weak base with a pKb=3.35. Consider the titration of 30.0mL of .030M of Methyl amine with 0.025M HCl. a) Write the appropriate equation for the reaction. b) Calculate K for the reaction in part (a). c) Calculate pH of the initial methyl amine solution (0mL ...
Friday, April 19, 2013 at 11:44am by Joe

Chemistry
Calculate the pH of the 0.20 M NH3/0.25 M NH4Cl buffer. I calculated the pH to be 9.15 What is the pH of the buffer after the addition of 10.0 mL of 0.10 M HCl to 72.5 mL of the buffer?
Tuesday, March 19, 2013 at 3:14pm by Cam

chemistry
A 50.00ml sample of 0.200M hydroflouric acid (HF) is titrated with 0.200M NaOH. The Pka of HF is 3.452. a) calculate the pH of the HF solution before titration b) calculate the pH after the addition of 20.00ml of NaOH
Saturday, November 6, 2010 at 5:04pm by michelle

chem
According to my table, bromocresol green changes pH between 3.8 and 5.4. You can calculate the approximate pH for the equivalence point for CH3COOH vs NaOH and that is about 8.5 or so. What do you think?
Tuesday, November 23, 2010 at 10:13pm by DrBob222

ap chemistry
for the following, mix the equal volumes of one solution from group I with one solution from group II to achieve the indicated pH. calculate the pH of each solution. Group I: .2M NH4Cl, .2M HCl, .2M C6H5NH3Cl, .2M (C2H5)3NHCl Group II: .2M KOI, .2M NaCN, .2M KOCl, .2M NaNO2 a...
Thursday, February 9, 2012 at 12:17am by hannah

A.P. Chemistry
pH = pKa + log [(base)/(acid)] You know Ka. Calculate pKa. NO2^- is the base. HNO2 is the acid. First, plug in pH = 3.00, the pH of the solution you want, and calculate the (base)/(acid) ratio. That gives you (base) = factor x (acid). Then you know mLbase*Mbase = mLacid*Macid ...
Saturday, April 3, 2010 at 5:05pm by DrBob222

Chem
pH = -log(H^+). Since the pH is a log function, the H^+ from 1 pH to the next (either higher or lower) is in steps of 10. That is pH = 2 is 10x weaker than a pH of 1 and 10x stronger than a pH of 3
Tuesday, May 4, 2010 at 8:26pm by DrBob222

Chemistry
A = pH of 8. 1,000 times means difference in pH of 3. If it is more H^+, then pH = 5 for the new solution. Is that acid or basic. pH<7 = acid pH=7 = neutral pH>7 = basic
Monday, November 14, 2011 at 3:56pm by DrBob222

science HElp
Ph scale Which on is true A substance with ph is twice as acidic as substance with ph of 4. A subtances with ph 3 is 10 as acidic as substance with ph of 4. A substance with ph 3 twice as alkies as substances with ph 4. a substancs with ph 3 10 time alkies as substance with ph...
Wednesday, November 23, 2011 at 7:14pm by shan

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