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April 21, 2014

Search: Calculate the pH after naoh is added

Number of results: 59,525

Chemistry
Hello, I need help with calculations for lab. I prepared excess NaOH and HCL solutions (unknown conc., ~0.1M). Then I standardized my NaOH solution by titrating known amounts of KHP (Potassium hydrogen phthalate)with it in the presence of phenolphthalein (indicator turns pink ...
Sunday, September 20, 2009 at 2:05pm by Pavel

CHEM!
Okay well I suddenly got confused for a lab I did We took pH meter than we calibrate it. Then we measure the pH of the acetic acid solution, which was used to determine the Ka of the acetic acid using the first method. We made a 1M solution of NaOH which was used to titrate 50...
Wednesday, May 9, 2007 at 6:05pm by Linda

chemistry
a and c are done the following. NaOH is a strong base which means OH^- = (NaOH). Then pOH = -log(OH^-) and pH + pOH = pKw = 14 For b, note that (NaOH) is very small and you need to take OH^- from H2O into account.
Saturday, May 4, 2013 at 2:02pm by DrBob222

chemistry
mols HCl = M x L = ? mols NaOH = M x L = ? Subtract, the one in excess will determine the acidity/basicity. If acid then pH = -log(HCl). If basic then pOH = -log(NaOH), then convert to pH.
Wednesday, May 2, 2012 at 1:46pm 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

chem -please help!!!!!!!!!!!!
An unknown compound, X, is though to have a carboxyl group with a pKa of 2.0 and another ionizable group with a pKa between 5 and 8. When 75 mL of 0.1M NaOH is added to 100 mL of a 0.1M solution of X at pH 2.0, the pH increases to 6.72. Calculate the pKa of the second ...
Monday, September 10, 2012 at 11:12pm by ron

Science
For NaOH, this is 100% dissociated; therefore, (OH^-) = (NaOH) OH^- = 2 M pOH = -log(OH^-) pH + pOH = pKw = 14. You know pOH, solve for pH. The H2SO4 isn't as simple as it lookis. If you are an advanced student, (0.39+x)/(0.39-x) = k2 for H2SO4. Solve for x and evaluate 0.39+x...
Sunday, February 9, 2014 at 5:49pm by DrBob222

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
calculate the change in pH when 9.00ml of 0.100M HCl(aq) is added to 100.0mL of a buffer solution that is 0.100M in NH3(aq) and 0.100M NH4Cl(aq). ...Calculate the change in pH when 9.00,L if 0.100M NaOH(aq) is added to the original buffer solution.
Sunday, October 28, 2012 at 5:18pm by mike

Chem Webwork
Complete the table below: What are the pH values if you take into account that the 8.00 mL of 0.10 M Acid was first diluted with 100 mL of water (like it will be in the experiment you perform in lab)? mL NaOH: 0.70 pH w/ HCl: 2.14 pH w/ HC2H3O2: ??? I got pH w/ HCl, but I can'...
Monday, April 25, 2011 at 4:25pm by Michelle

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
Okay so I did this problem, but it seems wrong? I put the answers I got... Determine the pH of the following tiration at each of the points indicated. A 71.7 mL solution of 0.182 M NaOH is titrated with 0.2086 M HCL. 1.) initial pH= is it 7.86 or 8.51? 2.) after addition of 10...
Sunday, October 9, 2011 at 12:57pm by help meeee pleaaseee

chemistry
how do you solve this? What is the pH of the solution created by combining 12.30 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of the 0.10 M HC2H3O2(aq)? mL NaOH pH wHCl pH wHC2H3O2 12.30 Complete the table below: What are the pH values if you take...
Monday, July 12, 2010 at 1:05am by Jin

Chemistry
Calculate the pH at the equivalence point in titrating a 0.120 M solution of NaHCrO4 (sodium hydrogen chromate) with 7.010−2 NaOH.
Saturday, November 20, 2010 at 1:31am by Josh

Chemistry
Calculate the pH at the equivalence point in titrating 0.110 M solution of sodium hydrogen chromate (NaHCrO4) with 8.010−2 M NaOH.
Sunday, April 22, 2012 at 12:28am by Kaitlyn Smith

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
I just did a lab on Acids and Bases and I am having trouble with the lab questions I was given to complete. Concentration of NaOH: 0.09999 M Volume of NaOH: 3.25 mL # moles of NaOH: 0.325 moles Initial Concentration of Weak Acid: ? (How do we calculate this) Part 2: Hydrolysis...
Sunday, March 29, 2009 at 1:53pm by Lalu

Chemistry
A. Na2O + HOH ==> 2NaOH B. There is a long way and a short way of doing this. The long way is to make a stoichiometry problem out of it, convert g Na2O to moles, calculate moles NaOH formed, then use M = moles/L. A shorter way is to forget about stoichiometry and reason it ...
Sunday, November 21, 2010 at 5:03pm by DrBob222

Chemistry
25 mL 0.1 M acetic acid is titrated with 0.1 M NaOH. Calculate the pH after the addition of 0.0 mL, 1.0 ml, 2.5 mL, 4.0 mL, 7.0 mL, 10.5 mL, 15.0 mL, 17.0 mL, 20.0 mL, 22.0 mL, 23.0 mL, 23.5 mL, 24.0 mL, 24.25 mL, 24.5 mL, 24.75 mL, 25.0 mL, 25.25 mL, 25.5 mL, 25.75 mL, 26.0 ...
Monday, April 22, 2013 at 4:34am by smartkid <33

Chemistry
KHP + NaOH ==> NaKP + H2O So 1 mole KHP uses 1 mole NaOH. moles KHP = grams/molar mass. Calculate moles KHP Then moles NaOH = moles KHP M NaOH = moles NaOH/L NaOH. (mL NaOH used = final reading - initial reading, then convert to liters.)
Tuesday, October 4, 2011 at 8:50pm by DrBob222

Chemistry
This is not a simple question. 1. Use the Debye-Huckel relationship to calculate the pH of 0.01M HCl. That is not the simple pH = -log(0.01) = 2 2. Now do the same for the mixture of 0.01M HCl and 5.80g NaCl after converting NaCl to mols then to M. 3. Solve for delta pH.
Friday, February 14, 2014 at 6:05pm by DrBob222

Chemistry
1. Calculate the pH for each of the following cases in the titration of 25.0 mL of 0.240 M pyridine, C5H5N(aq) with 0.240 M HBr(aq): (a) before addition of any HBr (b) after addition of 12.5 mL of HBr (c) after addition of 22.0 mL of HBr (d) after addition of 25.0 mL of HBr (e...
Thursday, February 20, 2014 at 7:06pm by Mia

chemistry
Prepare 500mL of a 0.200 M acetate buffer at pH 4.90 using only pure acetic acid, 3M NaOH, and water. 1) Add acetic acid to ~400mL of water in a 500 mL beaker. How many grams of acetic acid are needed? 2)Add 3 M NaOH solution until pH is 4.90. What volume of NaOH is needed? (...
Monday, September 5, 2011 at 11:58am by Ryn

Analy Chem
Find mols NaOH, subtract mols HBr. If mols NaOH are greater then pOH = -log(OH^-) and convert to pH by pH + pOH = pKw = 14. If mols HBr are in excess, pH = -log(H^+). Those three steps will do all of the points except for the equivalence point. That one is done by the ...
Wednesday, April 11, 2012 at 6:54pm by DrBob222

Chemistry
mols HCl initially = 0.025 x 0.1 = 0.0025 To end up with pH = 3 (0.001M H^+) we want H^+ to be 1E-3. If we work in millimols and let x = mL of 0.1M NaOH, we have then [(25.00 x 0.1M)-(0.1x)/(25+x)] = 1E-3M Solve for x and I obtained approx 24.5 mL of 0.1M NaOH that must be ...
Wednesday, February 26, 2014 at 7:44pm by DrBob222

Chemistry
Calculate the pH at the equivalence point in titrating a 0.120 M solution of NaHCrO4 (sodium hydrogen chromate) with 7.010−2 NaOH. Please help!
Saturday, November 20, 2010 at 10:43am by Josh

Introductory Chemistry
In a titration 25.1ml of a monoprotic weak acid is neutralized with 25.1 ml of .502M NaOH(aq). Calculate the Ratio of [A-] to [HA] after 12.55 of the .502 M NaOH has been added to the initial amount of HA. Anyone have any idea what's going on. I got as far as to find the mol's...
Wednesday, February 4, 2009 at 8:12pm by Nina

chemistry
What is the pH of the solution created by combining 2.80 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of the 0.10 M HC2H3O2(aq)? mL of NaOH pH w/HCl pH w/HC2H3O2 2.80 ? ? okay, so i tried m1v1=m2v2 and when i got m2 i would input it in -log(H+) to...
Wednesday, July 9, 2008 at 12:19am by UN

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

Chemistry-need help ASAP
I'll get you started but I don't believe you can't do any of it. I don't know what the problem is asking for when it says "difference in pH". Difference in pH from WHAT? 15 mL of 3M NaOH added to 500 mL. (NaOH) = 3M x (15/515) = ? (Note: This assumes the volumes are additive...
Monday, April 14, 2014 at 8:40pm by DrBob222

Chemistry
What is the pH of the solution created by combining 1.30 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? This is how I would go about solving the problem, but could you tell me where I went wrong? First I would find the number of mols of OH from NaOH and then use...
Sunday, May 4, 2008 at 3:02am by Marie

chemistry
Consider a 20.0mL sample of 0.105M HC2H3O2 is titrated with 0.125M NaOH. Ka=1.8x10^-5. Determine each of the following: a) the initial pH b) the pH at 5.0mL of added base c) the pH at one-half of the equivalence point d) the pH at the equivalence point
Monday, November 15, 2010 at 12:20am by bobjahng2

chemistry
The Ka values of maleic acid, HOOCCHCHCOOH, are shown below. Ka1 1.5 10-2 Ka2 2.6 10-7 A 50.0 mL sample of 0.11 M of maleic acid is titrated with 0.14 M NaOH. Calculate the pH at the following points in the titration curve. find the first and second eq point pH i thoguth i was...
Sunday, March 8, 2009 at 1:40am by Amy

CHEMISTRY
A student needed to standardize a solution of NaOH which was approximately 0.125 M. The student carefully prepared the titration setup, but after 25 mL of NaOH was added, what was the pH of solution if initially flask contains 25 mL of 0.250 M HCl solution?
Sunday, October 17, 2010 at 4:50pm by Maria

chemistry
A student needed to standardize a solution of NaOH which was approximately 0.125 M. The student carefully prepared the titration setup, but after 25 mL of NaOH was added, what was the pH of solution if initially flask contains 25 mL of 0.250 M HCl solution?
Sunday, October 17, 2010 at 6:51pm by Cindy

Chemistry
Start with the equation for the reaction NaOH + H2SO4 -> Na2SO4 + H2O which you need to balance. Then from the equation how many moles of NaOH react with each mole of H2SO4? Calculate number of moles of H2SO4 used (M) M=0.1 x 1 M = How many moles of NaOH needed? (N) ...
Tuesday, September 28, 2010 at 5:02am by Dr Russ

Chemistry
From what you've said, I think the teacher has TOLD you that the HCl s/he has provided is 0.1046 N. And if you've used 10.15 mL (0.01015 L), the # equivalents of HCl is L x N = 0.1046 x 0.01015 = ? Next, I assume you are to calculate the N of the NaOH listed next at 10 mL (0....
Saturday, March 3, 2012 at 9:35am by DrBob222

General Chemistry
millimoles HCl = 8.00 mL x 0.1M=0.8mmols. mmoles NaOH = 2.50 mL x 0.1M = 0.25 mmols. mmoles NaOH = 9.50 x 0.1M = 0.95 mmoles. mmoles HAc = 8.00 mL x 0.1M = 0.8 mmoles. -------------------------------------- ..........HCl + NaOH ==> H2O + NaCl initial...0.8....0........0...
Sunday, November 6, 2011 at 9:28pm by DrBob222

CHEMISTRY
A BUFFER SOLUTION IS MADE FORM 0.10 MOLES NaF AND 0.25 MOLES OF HF IN 1 LITER OF WATER ----WHAT WILL THE BUFFER CAPACITY BE IF 1.0M HCL IS ADDED -----WHAT IF 2.0 M OF NAOH IS ADDED?? PLEASE HELP I HAVE NO CLUE WHERE TO EVEN BEGIN!!! Calculate the pH of the solution using the ...
Tuesday, February 27, 2007 at 11:12pm by BRITTANY

Chemistry
Calculate the pH of a solution that is 2.00 M HF, 1.00 M NaOH, and 0.704 M NaF. (Ka = 7.2 E -4)
Wednesday, December 17, 2008 at 1:43pm by Schanee

chemistry
calculate the ph of 20 ml of .1M NaOH to 40 ml of acetic acid
Thursday, March 29, 2012 at 12:57am by mark

chemistry
calculate the ph of 20 ml of .1M NaOH to 40 ml of acetic acid
Thursday, March 29, 2012 at 1:10am by mark

chemistry
calculate the ph of 20 ml of .1M NaOH to 40 ml of acetic acid
Thursday, March 29, 2012 at 1:25am by mark

chemistry
calculate the ph of 20 ml of .1M NaOH to 40 ml of acetic acid
Thursday, March 29, 2012 at 1:26am by mark

chemistry
The reaction between the added solid and NaOH is: NaH2PO4 + NaOH --> Na2HPO4 + H2O 10.0gNaH2PO4 /120.0g/mol = 0.0833 moles NaH2PO4 initially. In the rection, the limiting reactant is NaOH. (0.150 L)(0.20 mol/L) = 0.030 mol NaOH 0.030 moles of NaOH ---> 0.030 moles ...
Wednesday, October 7, 2009 at 8:55pm by GK

Chem
Usually these don't come out the same and I didn't do the calculation in my head. Probably I should have. Since moles HCl = moles NaOH, neither is in excess and you have prepared some NaCl in water. So you have, except for the NaCl, which won't change the pH, just water. Water...
Sunday, November 28, 2010 at 9:00pm by DrBob222

Chem
Complete the table below: Note: Make simplifying assumptions, do not use the quadratic formula. What is the pH of the solution created by combining 1.90 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of the 0.10 M HC2H3O2(aq)? mL NaOH: 1.90 pH w/HCl...
Monday, May 7, 2012 at 1:07pm by Jenna

Chemistry
Why does the addition of 50ml of 0.5M NaOH to 50mL of 0.6M KOH cause the pH to decrease (aka more acidic)? Because you have reduced the (OH^-) of the 0.6 M KOH by adding an equal volume of 0.5 M NaOH 50 mL x 0.6 M KOH = 30 millimols. pH = 13.78 Adding 50 mL x 0.5 M NaOH = 25 ...
Tuesday, August 21, 2007 at 7:34am by Vic

Chemistry (Acids and Bases)
I just did a lab on Acids and Bases and I am having trouble with the lab questions I was given to complete. Concentration of NaOH: 0.09999 M Volume of NaOH: 3.25 mL # moles of NaOH: 0.325 moles Initial Concentration of Weak Acid: ? (How do we calculate this) Part 2: Hydrolysis...
Sunday, March 29, 2009 at 1:54pm by Lalu

Chemistry 2
mols NaOH = grams/molar mass M NaOH = mols/L solution M OH^- = M NaOH pOH = -log(OH^-) pH + pOH = pKw = 14.
Friday, February 21, 2014 at 2:30pm by DrBob222

Chemistry
How do you calculate the number of moles of NaOH to add to a liter of 1M NH4CL (pka of NH4+ = 9.25 ) to produce a solution buffering the pH at 8.75 ? thanks
Wednesday, June 29, 2011 at 2:45am by Lauren

AP CHEMISTRY
Calculate the pH at the equivalence point in titrating 0.100 M solutions of each of the following with 0.080 M NaOH. A) benzoic acid (C6H5COOH) Ka= 6.3*10^-5 for it
Thursday, March 1, 2012 at 4:26pm by DAN

CHEM
Are you sure that's 0.900 M NaOH? and not 0.0900 M? I'll assume 0.900 is correct. And I'll write acetic acid, HC2H3O2, (or CH3COOH) as HAc. Millimols HAc initially = 25 x 0.1 = 2.5. millimols NaOH added = mL x 0.900 The first thing to do is to determine the equivalence point. ...
Monday, October 1, 2012 at 12:54pm by DrBob222

chemistry
Calculate the pH when 75.20 mL of 0.114 M HCl is titrated with 0 ml of 0.108 M NaOH
Wednesday, March 21, 2012 at 3:24pm by blair

chemistry
Calculate the pH when 75.20 mL of 0.114 M HCl is titrated with 0 ml of 0.108 M NaOH
Wednesday, March 21, 2012 at 7:34pm by blair

Physics
Calculate the pH of a solution obtained by mixing 100cm3 of 0.1M HCl and 100cm3 of 0.2M NaOH
Thursday, January 31, 2013 at 3:50pm by Amarachukwu

Physics
Calculate the pH of a solution obtained by mixing 100cm3 of 0.1M HCl and 100cm3 of 0.2M NaOH
Thursday, January 31, 2013 at 3:51pm by Amarachukwu

Science
Calculate the PH of and POH of the following solution and comment on them.(a)0.39 moldm3 of H2SO4(b)2.0 moldm3 of NaoH
Sunday, February 9, 2014 at 5:48pm by Oladimeji Taofeek

Science
Calculate the PH of and POH of the following solution and comment on them.(a)0.39 moldm3 of H2SO4(b)2.0 moldm3 of NaoH
Sunday, February 9, 2014 at 5:49pm by Oladimeji Taofeek

AP Chemistry
help with acid/bases If the pH at 50.0 mL of NaOH added is 4.0 and the pH at 150.0 mL of NaOH added is 8.0, determine the values Ka1 and Ka2 for the diprotic acid. Ka1 i dotn know how to start, please help!
Wednesday, March 11, 2009 at 12:50am by Amy

For Dr.Bob222 (chem work)
What is the pH of a solution of 120 ml 0.15M acetic acid to which we add 30mL 0.2M NaOH? CAN YOU CHECK MY WORK PLEASE? 0.15 mol/L * 0.12 L = 0.018 mol acetic acid 0.2 mol/L * 0.03 L = 0.006 mol NaOH 0.018 - 0.006 = 0.012 mol of acetic acid in excess pH = pKa + log (acid/base) ...
Monday, August 27, 2007 at 11:17pm by Gulzaman

Titration
This is the titration of a strong base with a strong acid. Begin: 100 mL x 0.100M NaOH = 10 millimoles. millimoles HBr added = 1.00M x mL = ? .............NaOH + HBr ==> NaBr + H2O initial......10mmol...0.......0......0 added.................0 change........-0............ ...
Monday, January 23, 2012 at 3:46pm by DrBob222

chemistry
A 20.0 gram sample is a mixture of sodium phosphate ,sodium mono-hydrogen phosphate,sodium dihydrogen phosphate and sodium chloride. The sample is dissolved in 100.0 ml of deionized water and titrated with 1.5 M hydrochloric acid. The initial pH of the solution is pH= 12.9. ...
Tuesday, May 22, 2012 at 6:11am by bill

chemistry
A 20.0 gram sample is a mixture of sodium phosphate ,sodium mono-hydrogen phosphate,sodium dihydrogen phosphate and sodium chloride. The sample is dissolved in 100.0 ml of deionized water and titrated with 1.5 M hydrochloric acid. The initial pH of the solution is pH= 12.9. ...
Tuesday, May 22, 2012 at 6:41pm by bill

chemistry
If 25.00 mL of 0.20 mol/L HCO2H(aq) is titrated with 0.20 mol/L NaOH(aq) (the titrant), determine the pH a) befor titration began b)after 10.00 mL of NaOH has been added c) at the equivalence point
Saturday, April 5, 2008 at 8:39pm by Bradely

pH- really hard one
What is the pH of the solution created by combining 1.00 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of the 0.10 M HC2H3O2(aq)? NaOH + HCl ==> NaCl + H2O So all the NaOH is neutralized leaving NaCl, which will not affect the pH either way, ...
Sunday, April 15, 2007 at 7:39pm by Christine

science
I added 40 mL of NaOH 1N to rise the pH of 10g teriphitalic acid from 5.3 to 6.3, so if I adde the same 40 mL of NaOH to 12g of the same acid what is the new pH will I have?
Friday, January 22, 2010 at 4:06pm by Jack

chemistry
Calculate the pH of a solution obtained by mixing 30 mL of 0.75 M CH3COOH with 15 mL of 1.5 M NaOH.
Tuesday, January 24, 2012 at 9:58pm by grewal

chemistry
a) before titration begins. That is a 0.2 M solution of HCOOH. HCOOH ==> H^+ + HCOO^- (HCOOH) = 0.2-x (H^+) = x (HCOO^-) = x Ka = (H^+)(HCOO^-)/(HCOOH) Plug the above variables into Ka and solve for (H^+), then convert to pH. b) after 10.00 mL NaOH has been added. HCOOH + ...
Saturday, April 5, 2008 at 8:39pm by DrBob222

chemistry
moles NaOH = grams/molar mass M NaOH = moles NaOH/L solution. (OH^-) = (NaOH) pOH = -log(OH^-), then convert to pH by pH + pOH = pKw = 14'= Technically, this is not the correct answer. Technically, the correct answer cannot be obtained UNLESS one knows the density of the ...
Thursday, February 24, 2011 at 11:37pm by DrBob222

CHEMISTRY (WEBWORK)
You have two problems here. The first is the combination of NaOH and HCl. Work with that one first. The second one is NaOH and HC2H3O2. Work with that one second. For the first one, 1. Write the balanced equation. 2. Calculate moles NaOH and moles HCl. moles = M x L. 3. ...
Monday, July 12, 2010 at 6:19pm by DrBob222

chemistry
No. Isn't the first column mL NaOH and the second column is pH. Then between pH 6.5 and 11.2 or so is the vertical portion of the pH and that occurs about 12 mL or so if I read your numbers correctly. A pH of 12 is at 15.0 mL and the curve in that region is almost horizontal.
Saturday, April 5, 2008 at 5:22pm by DBob222

Chemistry, #3
Thallium hydroxide is a strong base used in the synthesis of some organic compounds. Calculate the pH of a solution containing 2.55 g TIOH per liter. Sorry! I'm having a really hard time with this acid/base stuff! TlOH is a strong base as the problem says. Do it just as you ...
Saturday, August 4, 2007 at 4:47pm by Taasha

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 (heat flow, simple)
Well I know to calculate heat flow you use, q=ms delta t. for this experiment we mixed naoh with hcl into water. the total mass (volume) of the mixture was 100g the temperature change for naoh was 11.7 degrees C and for hcl it was 11.8 degrees C now im looking to calculate ...
Friday, March 12, 2010 at 8:00am by Abdullah

Chemistry
The basic problem here is that you are trying to use the Henderson-Hasselbalch buffer equation to solve a problem that is not a buffer. Your solution is not a buffered solution problem. There is an excess of NaOH when reacted with HCl and the pH is determined by the excess OH ...
Monday, May 3, 2010 at 2:50pm by DrBob222

chemistry
Run # Volume NaOH used (mL) 1 4.1 2 4.3 3 2.8 Concentraion of NaOH: 0.113 M pH of acid: 2.84 the questions are: #moles of NaOH: ? initial acid concentration: ? Determine the Ka and pka of the weak acid: ? So here is what I did: Shaked for several minutes about 1 g of the acid ...
Sunday, July 15, 2012 at 7:53pm by fenerbahce

chemistry- pH, neutralization
What volume of NaOH was required to have neutralized the HCl. HCl + NaOH --> H2O + NaCl There no other information given in the problem except in later questions like the NaOH had 0.1 M and that there was 50.00 mL of HCl.
Thursday, February 2, 2012 at 3:49pm by laura

chemistry
The whole idea here is that you have an equation that tells you what is going on AND you have measured quantities of each; therefore, you can calculate the missing quantity of the other one. 2NaOH + H2SO4 ==> Na2SO4 + 2H2O How many moles acid did we use? That is M x L = ? ...
Friday, March 16, 2012 at 12:15am by DrBob222

Chemistry
44.70 ml of 0.100 M NaOH are required to completely neutralize 50.00 ml of a weak monoprotic acid, HA. When 34.43 ml of NaOH are added to another 50.00 ml of the acid, the pH reading was 4.80. Calculate Ka for the acid using the partial neutralization method.
Saturday, April 9, 2011 at 2:49pm by Cassie

Chemistry
Calculate the pH at the equivalence point when 50 mL of 0.098 M propionic acid is titrated with 0.340 M NaOH. I tried solving for the volume of NaOH and them using the total volume and then plugging it in to [H+][A-]/[HA] and used the Ka value for propionic acid but it was not...
Monday, April 15, 2013 at 7:18pm by Maddie

chemistry
mols NaOH = M x L mols CH3COOH = mols NaOH. mols CH3COOH = M x L You took 25 mL, you measure the mols CH3COOH, calculate M CH3COOH. I presume you are to graph the results. I don't know what instructions you have been given but you must find the equivalence oint for the ...
Tuesday, April 8, 2008 at 11:39pm by DrBob222

chemistry
1)100ml sample of solution that is 0.2m in both Naf and Hf has 4.0 ml of 1.0m hcl added to it. calculate the ph change of this soultion .ka =7.2*10^-4 2)40 ml of 0.32m benzoic acid if titrated with 60 ml of 0.2 m naoh. clacilate the ph of the resulting solution at the ...
Sunday, March 4, 2012 at 6:28pm by Anonymous

chemsitry
1)100ml sample of solution that is 0.2M in both Naf and Hf has 4.0 ml of 1.0M hcl added to it. calculate the ph change of this soultion .ka =7.2*10^-4 2)40 ml of 0.32M benzoic acid if titrated with 60 ml of 0.2 M naoh. clacilate the ph of the resulting solution at the ...
Sunday, March 4, 2012 at 7:24pm by Anonymous

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
A buffer containing 1.2169 M of acid, HA, and 0.1431 M of its conjugate base, A-, has a pH of 3.96. What is the pH after 0.0017 mol NaOH is added to 0.5000 L of this solution? I can't figure this out for the life of me, i'm sure its just some simple mistake i'm making but can ...
Monday, April 2, 2007 at 1:00pm by Rafael

chemistry AP
This problem is a little confusing because of the wording; i.e., it isn't easy to tell when we are talking about system 2 and when we aren't. The best buffer to use is one that has pKa = pH you want for the solution. So convert Ka for each system to pKa. I get something like ...
Sunday, March 28, 2010 at 1:56am by DrBob222

chemistry
i have 1m3 of water at ph 5 how many ml of NaOH I need to add to get ph 7
Wednesday, April 20, 2011 at 1:46am by nabeel

Chemistry
NaOH + HC2H3O2 ==> NaC2H3O2 + H2O moles NaOH = M x L = ?? moles HC2H3O2 = M x L = ?? See which is in excess when NaOH is added to HC2H3O2. If NaOH is in excess the pH is determined by excess OH. If HC2H3O2 is in excess, then you have a mixture of acetic acid and sodium ...
Saturday, May 1, 2010 at 8:43pm by DrBob222

chemistry
calculate the volume of 0.1M NaOH which must be added to 50 mL of 0.1M HCl to give a final solution of pH 6???
Thursday, March 4, 2010 at 12:35am by sara

science
Calculate the pH at 0, 10, 90, 100 & 110% titration for the titration of 50.0ml of 0.1M HCl with 0.10M NaOH?
Thursday, January 10, 2013 at 4:46pm by Eline

Chemistry
Calculate the pH of a solution that is 2.00M HF, 1.00M NaOH, and 0.393M NaG (Ka=7.2 x10^-4). The answer I got was 4.76 ..
Friday, March 22, 2013 at 9:45pm by Jill

Chemistry
Calculate the volume of .100M NaOH that must be added to reach ph of 3 in the titration of 25.00 mL of .100M HCl
Wednesday, February 26, 2014 at 7:44pm by Chemist in progress

biochemistry
Calculate the pH of the resultant solution of mixing together two solutions of 2 L of 1.0 M acetic acid, 0.5 L of 1.0 M sodium acetate and then adding 8 g of solid NaOH (MW = 40.0 g/mole).
Thursday, January 17, 2013 at 4:46pm by Dre

chemistry
Write the equation. Calculate mols HCl present Determine mols NaOH needed. Calculate mL NaOH required. Post your work if you get stuck.
Sunday, April 6, 2008 at 2:07am by DrBob222

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
NaOH is a strong base. As such it is 100% ionized; therefore, if pH = 10 then pOH = 4, and use pOH = -log(OH^-) to calculate (OH^-) in moles/L = molarity. Then M = moles/L. You know M and L, calculate moles. Finally, moles = grams/molar mass. Solve for grams.
Tuesday, September 7, 2010 at 12:00pm by DrBob222

chemistry
how much of 0.1 M NaOH is needed to neutralize 5mL of 0.1 M of HCL to a ph 7(color on the ph scale)...Thank you
Tuesday, May 14, 2013 at 1:07pm by mae

Chemistry
You weighed KHP. Calculate the moles KHP you titrated with NaOH. Moles KHP = grams/molar mass. You should write the equation for KHP + NaOH but it is a 1:1 ratio (1 mole KHP to 1 mole NaOH). Therefore, moles KHP titrated will equal moles NaOH used. Then you know M x L = moles ...
Sunday, September 20, 2009 at 2:05pm by DrBob222

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