Wednesday
April 16, 2014

Search: NaOH, HC2H3O2

Number of results: 4,863

Chemistry
oh no that was a type it's actually .20M NaOH so that gives me: n = c* v = .2mol/L * .025L = .005 moles HC2H3O2= c*v = .1 * .05L = .005 I still get the same moles for both of them!
Monday, August 10, 2009 at 12:12pm by Anonymous

biology
suppose 23mL of NaOH was required. How much Carbonic Acid was neutralized? 1L of .01 NaOH contains ____ mol NaOH? lmL of .01 NaOH contains _____mol NaOH? 23mL of .01 NaOH contains _____ mol NaOH? 2 mol of NaOH react with 1 mol H2CO3 2.3 x 10^-4 mol of NaOH react with ____mol CO2
Tuesday, October 5, 2010 at 6:03pm by Anonymous

chemistry
HAc is HC2H3O2. HAc is so much easier to write than HC2H3O2.
Tuesday, November 29, 2011 at 4:47pm by DrBob222

chem lab (webwork)
What is the pH of the solution created by combining 1.80 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 NaOH pH wHCl pH wHC2H3O2 1.80 Complete the table below: What are the pH values if you take into account that the 8....
Tuesday, April 13, 2010 at 9:36pm by anonymous

chem.
Ok, so far this is what i've done. A. to get moles of NaOH, i multiplied 0.5062M x 0.01658L=8.39x10^-3, then i divided this number by .010L, i got .8392M B. (8.392x10^-3)x(60.052g HC2H3O2)=.5039g, after this part i got stuck.
Friday, March 7, 2008 at 12:33pm by aditya

chemistry grade 11
(avg. ammount of substance) ( 28.0 mL + 27.3 mL + 27.5 mL ) / 3 = 27.7 mL HC2H3O2 + NaOH => NaC2H3O2 + HOH n= M x L = 0.30 M x 0.0277 L = 0.00831 mols unknown:NaC2H3O2:x:1mol:NaC2H3O2:/ known:NaOH:0.00831 mols:1 mol:NaOH: x=0.00831 mol molar mass of HC2H302: H x 4 = 4.04 C ...
Monday, December 15, 2008 at 10:18pm by diana

chemistry
Given .300 L of a buffer solution that is .250 M HC2H3O2 and .50 M NaC2H302, what is the new pH if .0060 mol HCL is added? what about .0060 mol NaOH?
Sunday, December 5, 2010 at 8:58pm by Symone

Chemsitry
Hi I have done this problem like 15 times when I find the mole I get .8 for HCL and .23 for Naoh and the equilibrium conc i get is negative. then I plug it in and get it wrong. Can someone please help me? Complete the table below: Note: Make simplifying assumptions, do not use...
Friday, April 27, 2012 at 9:07pm by someone

chemistry 101
If 15g of NaOh is dissolved in 285 g of water, calculate the following. Assume the density of the solution is 1.06 g/cc. a) Calculate the moles of NaOH in the solution? My answer is 15gNaOH/40g NaOH= .0375 mole NaOH b) Waht is the mass % w/w of the solution? My answer is 15g ...
Saturday, December 8, 2012 at 12:34am by Tracy

chemistry
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 What are the pH values if you take into account that the 8.00 mL of 0.10 M Acid was...
Monday, May 5, 2008 at 5:31am by Renee

chemistry
Do mean to calculate the volume of NaOH required for the neutralization? 2NaOH + H2SO4 ==> Na2SO4 + 2H2O moles H2SO4 = grams/molar mass Use the coefficients in the balanced equation to convert moles H2SO4 to moles NaOH. 15% NaOH means 15 g/100 mL (is that 15% w/v?) So 15 g ...
Thursday, March 17, 2011 at 4:30pm by DrBob222

Chemistry(Please help, thank you!!)
2NaOH + H2SO4 ==> 2H2O + Na2SO4 moles H2SO4 = M x L = ? moles NaOH = 2 x moles H2SO4 from the equation. M NaOH = moles NaOH/L NaOH. You have moles NaOH and L NaOH, solve for M NaOH.
Tuesday, October 25, 2011 at 10:21pm by DrBob222

chemistry
which of the following was not one of the products when you titrated the vinegar solution with sodium hydroxide? HC2H3O2+NaOH===>NaC2H3O2+H2O a salt water sodium acetate acetic hydroxide
Tuesday, July 13, 2010 at 4:05pm by Anonymous

Inorganic chemistry
mol KHP = (0.7719g)(1 mol KHP/204.2g) = .0038mol Where are the moles of NaOH? I know that there are 0.02637 L of NaOH and I know M = mol/l I know there are 40g NaOH/mol NaOH There is 1 mol of NaOH in the balanced equation But I do not have grams of NaOH
Tuesday, April 14, 2009 at 1:02pm by Steve

chemistry
You must recognize that when adding NaOH to HC2H3O2 (which is acetic acid and I will call it HAc and use Ac^- for acetate ion), you are forming a buffered solution. That means use the Henderson-Hasselbalch equation. HAc + NaOH ==> NaAc + H2O. moles HAc = 1.0 L x 2.0 M = 2 ...
Monday, April 12, 2010 at 9:18pm by DrBob222

AP Chemistry
H2A + NaOH ==> NaHA + H2O for the first H. NaHA + NaOH ==> Na2A + H2O for the 2nd H. mols H2SO4 = 0.018L x 0.122 M = ? mols NaOH = same for the first H. M NaOH = moles NaOH/L NaOH. Solve for L NaOH.
Saturday, March 17, 2012 at 2:08am by DrBob222

Chemistry
Are you titrating the ASA with NaOH? If so use the volume NaOH in the titration. Then mols = M NaOH x L NaOH
Tuesday, June 4, 2013 at 12:29pm by DrBob222

Chemistry
1. What is the pH of the solution created by combining 0.50 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)? 2. 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...
Monday, November 1, 2010 at 12:14am by Kyo

AP Chemistry
moles acid or base = M x L = ?? Next use the coefficients in the balanced equation to convert moles acid/base to the other one. The M = moles/L. Here is an example using (a). HCl + NaOH ==> NaCl + HOH moles HCl = M x L = 0.500M x 0.021L = 0.0105. moles NaOH = 0.0105 x (1 ...
Saturday, September 24, 2011 at 9:11pm by DrBob222

chemistry
How many moles NaOH do you need? THat is M x L = ? M NaOH = moles NaOH/L NaOH. YOu know M NaOH (6.0M) and you know moles from the first part. Solve for L and convert to mL.
Monday, October 24, 2011 at 7:10pm by DrBob222

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 2 Lab
Because the part should be, (1 x 10^-3)^2/1.75 x 10^-5=HC2H3O2 (H3O+/HC2H3O2)*100, should give you the degree of ionization Flipped it by accident.
Tuesday, March 19, 2013 at 6:50pm by Devron

CHEMISTRY
calculate the ionization constant of the conjugate base for a solution made from 0.2Molar HC2H3O2 and 0.5Molar C2H3O2.The ionization constant for the acid (HC2H3O2) IS 1.8 Multiplied by 10^(-5)
Saturday, March 31, 2012 at 11:57am by laze

chemistry
What is the pH of the solution created by combining 0.80 mL of the 0.10 M NaOH(aq)with 8.00 mL of the 0.10 M HC2H3O2(aq)?
Monday, July 13, 2009 at 7:29pm by Anonymous

chemistry
What is the pH of the solution created by combining 12.00 mL of the 0.10 M NaOH with 8.00 mL of the 0.10 M HC2H3O2?
Saturday, April 24, 2010 at 10:41pm by need help please!!!

Chemistry
A certain vinegar is 6.02% acetic acid (HC2H3O2) by mass. How many grams of HC2H3O2 are contained in a 355-mL bottle of vinegar? Assume a density of 1.01g/mL.
Friday, February 19, 2010 at 6:06pm by lucylu

CHemistry
im not sure how u solve these types of problems... How many moles of NaOH are contained in 200ml of a 0.1M of NaOH? How many grams of NaOH are contained in 500ml of a .5M solution of NaOH? <<How many moles of NaOH are contained in 200ml of a 0.1M of NaOH? >> A 0.1 ...
Saturday, April 21, 2007 at 10:21pm by Phil

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 HC2H3O2(aq)? I got 1.3. is that correct?
Wednesday, April 29, 2009 at 9:18pm by ibob

chemistry
I think 1 is right. I disagree with 2. Yes, the solution of NaOH M is too low since all of the NaOH has not dissolved but during the second titration the NaOH is stronger which means it takes less NaOH than it should and M = mmols/mL so smaller NaOH mL means a larger M. 3. The...
Tuesday, March 11, 2014 at 2:25am by DrBob222

Chemistry
Write a balance ionic and net equation for the following: KOH + HC2H3O2 I came up with the following but think this is wrong: KOH + HC2H3O2 -> H2O (l) + KC2H3O2 (aq)
Friday, May 13, 2011 at 9:42pm by Thao

CHEM 111
What is the Ka value of acetic acid from the pH of the buffered solution? pH=4.39 of 25ml of HC2H3O2 with .410g NaC2H3O2 added. Ka = [H3O][C2H3O2] / [HC2H3O2]
Thursday, June 9, 2011 at 8:58pm by Anonymous

Chemistry105
mol NaOH = grams/molar mass= ? M = mols/L = ? mols/0.1L b) mols HCl = M x L = ? mols NaOH = mols HCl M NaOH = mols/L soln. You know M NaOH and mols NaOH, solve for L NaOH and convert to mL if you wish.
Tuesday, December 4, 2012 at 9:47pm by DrBob222

Chemistry
1. A good indicator will have a(n)____ close to this volume and pH. I think it's endpoint but it's wrong. 2. (part a) What is the pH of the solution created by combining 1.70 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)? ...
Saturday, April 28, 2012 at 3:38pm by Jody

chemistry
moles acrylic acid = grams/molar mass moles acrylic acid = moles NaOH. M NaOH = moles NaOH/L NaOH. You know M NaOH and moles NaOH, solve for L NaOH and convert to mL.
Wednesday, January 25, 2012 at 6:54pm by DrBob222

Chemistry
C7H6O3(s) + C4H6O3(l) → C9H8O4(s) + HC2H3O2(l) is the equation. At 20 degree celsius, how many liters of acetic acid, HC2H3O2, would be formed? The density of acetic acid is 1.05g/cm3.
Thursday, February 19, 2009 at 8:52pm by Emat

Chemistry
#1. For H2SO4L: 2NaOH + H2SO4 --> Na2SO4 + 2H2O moles H2SO4 = M x L = ?? moles NaOH = 2x moles H2SO4 (from the equation). M NaOH = moles NaOH/L NaOH. #1. For HCl: NaOH + HCl ==> NaCl + H2O moles NaOH = M(from the first part) x L moles HCl = moles NaOH (from the equation...
Monday, October 4, 2010 at 3:03pm by DrBob222

Chem 2 Lab
H3PO4 + 3NaOH ==> 3H2O + Na3PO4 mols H3PO4 = 0.4/molar mass H3PO4 = ? Convert mols H3PO4 to mols NaOH using the coefficients in the balanced equation. M NaOH = mols NaOH/L NaOH. You know M and mols NaOH, solve for L NaOH
Wednesday, April 25, 2012 at 10:30pm by DrBob222

chemistry
HC2H3O2 ==> H^+ C2H3O2^- Ka = (H^+)(C2H3O2^-)/(HC2H3O2). Set up an ICE chart, substitute into the above Ka expression, and solve for H^+, then convert to pH. Post your work if you get stuck.
Monday, November 15, 2010 at 2:16pm by DrBob222

chemisrty
HCl + NaOH ==> NaCl + H2O mols HCl = M x L = ? mols NaOH = same. (Look at the coefficients in the balanced equation.) M NaOH = mols NaOH/L NaOH. You have molos and M, solve for L.
Thursday, April 25, 2013 at 11:47am by DrBob222

chemistry
What is the pH of a buffer solution made from 0.20M HC2H3O2 abd 0.5M C2H302^-.The ionization constant of the acid (Ka)(HC2H3O2)is 1.8multiplied by 10^-5. (ii)Calculate the ionization constant of its conjugate base
Monday, April 2, 2012 at 4:14am by lovemore

Chem
KHC8H4O4 + NaOH ==> NaKC8H4O4 mols KHC8H4O4 = grams/molar mass. mols NaOH = same (Look at the coefficients in the balanced equation.) M NaOH = mols NaOH/L NaOH
Monday, April 8, 2013 at 7:03am by DrBob222

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
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
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
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
HCl is titrated with NaOH. When doing the titration, some of the NaOH splashed onto the inside surface of the Erlenmyer flask, and you forgot to rinse it into your sample. Would the systematic error be falsely high, low, or unaffected and why? Thanks. As I understand the ...
Sunday, September 17, 2006 at 4:25pm by bria

Chemistry
NaHCO3 + HC2H3O2 ==> NaHC2H3O2 + H2O NaHCO3 is sodium bicarbonate (or sodium hydrogen carbonate is the more modern name). HC2H3O2 is acetic acid. Only the first H listed is acidic which is why they list it separately). This is like a long line of acid/base reactions. acid...
Friday, October 4, 2013 at 11:29pm by DrBob222

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

Chemistry
0.01L KHP * 0.445M KHP = 0.00445 molKHP KHP and NaOH are in 1 to 1 ratio so, moles NaOH = 0.00445 so, 0.00445mol NaOH/ 0.01154L NaOH = 0.386M NaOH
Monday, October 4, 2010 at 7:30pm by Andrew

Chemisty
How many mols MgSO4 so you have? That is moles = M x L = 0.541 x 0.148 = ? Using the cofficients in the balanced equation, convert moles MgSO4 to moles NaOH. That is ?moles MgSO4 x (2 moles NaOH/1 mol MgSO4) = ?moles MgSO4 x 2/1 = ? moles MgSO4. Then M = moles/L soln MNaOH = ...
Tuesday, February 7, 2012 at 9:39pm by DrBob222

Chemistry
moles H2C2O4 = grams/molar mass = ?? Using the coefficients in the balanced equation, convert moles H2C2O4 to moles NaOH. That will be ??moles H2C2O4 x (2 moles NaOH/1 mole H2C2O4) = ??moles H2C2O4 x 2 = xx moles NaOH. Then M NaOH = moles NaOH/L NaOH, and round to the ...
Tuesday, June 7, 2011 at 7:06pm by DrBob222

Chemistry
I really don't know how to approach this problem and I really need help. Using the average molarity of your initial acetic acid solutions, the initial volumes, and the volume of NaOH added to reach the equivalence point, calculate the [C2H3O2-] concentration at the equivalence...
Thursday, May 6, 2010 at 2:22pm by Megan

Chemistry
Develop a recipe for 1.00L of pH 4.50 buffer using only 17.4M HC2H3O2 and 3.00M NaOH (and deionized water). Be sure that it can accommodate an addition of at least .50 mol of strong acid or base with a change in pH less than/equal to 1.
Monday, December 12, 2011 at 5:20pm by Shana

chem 111 lab
KHP + NaOH ==> NaKP + H2O mols KHP = grams/molar mass From the equation, mols KHP = mols NaOH. M NaOH = moles NaOH/L NaOH
Monday, February 20, 2012 at 6:22pm by DrBob222.

chemistry
We'll call benzoic acid HB. HB + NaOH ==> NaOH mols HB = grms/molar mass Look at the equation (the coefficients) 1 mol NaOH = 1 mol HB; therefore, mols HB = mols NaOH. Then M NaOH = mols NaOH/L soln.
Wednesday, May 9, 2012 at 10:58pm by DrBob222

Chemisty
Vol NaoH titration Ml Naoh (1L/1000 mL) (.270 M (NAOH)= mol NaOH
Monday, January 14, 2013 at 5:11pm by Bellam

chemistry
Write the equation and balance it. HCl + NaOH ==> NaCl + H2O 1. moles HCl used = M x L = ?? 2. Using the coefficients in the balanced equation, convert moles HCl to moles NaOH. Since everything is a 1:1 ratio, that means moles NaOH = moles HCl. 3. Then M NaOH = moles NaOH/L...
Wednesday, June 15, 2011 at 2:07pm by DrBob222

AP chemistry
moles KHP = grams/molar mass Substitute and solve for mols. KHP + NaOH ==> NaHP + H2O so the reaction is 1:1 and moles KHP = moles NaOH. Then M NaOH = moles NaOH/L NaOH. To obtain L NaOH, you will need to subtract the final buret reading - initial buret reading and convert ...
Sunday, October 24, 2010 at 8:29pm by DrBob222

Chemistry
I find it helpful to write each step of the procedure and see how the question affects each. 1. mols KHP = grams/molar mass 2. mols NaOH = mols KHP 3. M NaOH = mols NaOH/L NaOH So you did steps 1 and 2 right but on 3 added too much L NaOH. That's in the denominator, too big ...
Wednesday, December 5, 2012 at 3:17pm by DrBob222

acid and base titrations
Which of the following solutions should be used when titrating a 25.00mL sample of CH3COOH that is approximately 0.1 M? a.) 0.150 M NaOH b.) 0.001 M NaOH c.) 3.00 M NaOH d.) 6.00 M NaOH
Sunday, November 21, 2010 at 5:15am by jj reddick

CHEMISTRY
mols HCl = M x L = ? mols NaOH = mols HCl (look at the coefficients in the balanced chemical equation). M NaOH = mols NaOH/L NaOH You know mols and L, solve for M. L for NaOH is 0.075 since you want M of the diluted solution.
Friday, October 18, 2013 at 1:38pm by DrBob222

Chemistry help
NaOH is a strong base, so it will completely dissociate into OH-. pOH+pH=14, so 14-pOH=pH Solve for pOH 2.00g of NaOH*(1 mole of NaOH/39.997 g)= moles of NaOH moles of NaOH/2.00L=molarity of NaOH -log[molarity of NaOH]=pOH 14-pOH=pH
Monday, July 29, 2013 at 7:36pm by Devron

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

organic bio chemistry
H2SO4 + 2NaOH ==>Na2SO4 + 2H2O mols H2SO4 = M x L = ?? Look at the coefficients in the balanced equation. mols NaOH = 2 x mole H2SO4. Then M NaOH = moles NaOH/L NaOH You know M and you know moles, solve for L NaOH and convert to mL.
Tuesday, March 8, 2011 at 11:06pm by DrBob222

Chemistry
moles solid NaOH = 9.4 g/molar mass NaOH = ?? moles NaOH solution = M x L = ?? Add to find the sum of the moles. This is the total NaOH dissolved (in moles). Now convert 2.37 gallons of water to mL and concn NaOH (molarity) = total moles/L.Post your work if you get stuck.
Monday, October 4, 2010 at 6:30pm by DrBob222

chem
KHC2O4 + NaOH ==> NaKC2O4 + H2O mols KHC2O4 = grams/molar mass = ? mols NaOH = mols KHC2O4(see the coefficients in the balanced equation). Then M NaOH = mols NaOH/L NaOH and solve for M
Wednesday, November 21, 2012 at 2:52pm by DrBob222

AP Chemistry
HCl + NaOH ==> NaCl + H2O mols HCl = M x L = ? mols NaOH = mols HCl M NaOH = mols NaOH/L NaOH I believe that works out to be about 4.2M but check my work.
Wednesday, September 11, 2013 at 6:18pm by DrBob222

chemistry
calculate the molarity of an acetic acid solution if 39.96 mL of the solution is needed to neutralize 136mL of 1.41 M sodium hydroxide. the equation for the reaction is HC2H3O2(aq) + NaOH(aq) > Na+(aq) + C2H3O2(aq) +H2O(aq)
Sunday, April 29, 2012 at 9:49pm by Randy

chemistry
calculate the molarity of an acetic acid solution if 39.96 mL of the solution is needed to neutralize 136mL of 1.41 M sodium hydroxide. the equation for the reaction is HC2H3O2(aq) + NaOH(aq) > Na+(aq) + C2H3O2(aq) +H2O(aq)
Sunday, April 29, 2012 at 9:49pm by Randy

chemistry
You need to learn to place an arrow; otherwise, we don't know the difference between the reactants and the products. In this case, how many mole HCl did you use? mole HCl = M x L = ?? Now convert, using the coefficients in the balanced equation, to moles NaOH. The equation is ...
Wednesday, June 22, 2011 at 6:43pm by DrBob222

chemistry
NaOH + KHP ==> NaKP + H2O mols KHP = grams/molar mass mols NaOH = mols KHP (look at the coefficients in the balanced equation.) M NaOH = mols NaOH/L NaOH
Tuesday, December 11, 2012 at 3:57pm by DrBob222

chemistry
It still makes no sense to me. Here is the problem as I see it. I don't understand what the 15% has to do with the problem. What is the mass of NaOH (notice I use caps since naoh means absolutely nothing) required to neutralize 176 g H2SO4. 2NaOH + H2SO4 ==> 2H2O + Na2SO4 ...
Saturday, March 19, 2011 at 10:40am by DrBob222

Chemistry
NaOH + KHP ==> NaKP + H2O moles KHP = M x L = ?? moles NaOH = same (from the equation) M NaOH = moles NaOH/L NaOH
Monday, October 4, 2010 at 7:30pm by DrBob222

chemistry
calculate the pH of a buffer solution containing 0.200M acetic acid, HC2H3O2, plus 0.150M sodium acetate. The dissociation constant for HC2H3O2 is 1.76 x 10-5 I dont think our instructor gave enough notes on these things Im kind of winging it from the book. Could you please ...
Friday, November 11, 2011 at 8:02pm by Monique

Chemistry.. help plz
3. How much 0.10 M Base (in mL) is required to neutralize 8.00 mL of the 0.10 M acid? Base Acid Base Volume (mL) NaOH HCl ____________ NaOH HC2H3O2 _____________ 4. How would the volume of base change from problem three if the 8.00 mL of 0.10 M Acid was first diluted with 100...
Thursday, May 1, 2008 at 12:31pm by Amy

Chemistry
I've been working on this problem for hours and cant figure it out. I know it should be simple, but I'm stuck... The question is... Describe how to prepare 1.00L of a 1.0% (w/v) NaOH from a 2.0 M NaOH. *I need to figure out how many ml of the stock solution is needed. So far I...
Thursday, January 10, 2013 at 6:08pm by James

chemistry
H3PO4 + 3NaOH ==> 3H2O + Na3PO4 mols H3PO4 = M x L = ? Using the coefficients in the balanced equation, convert mols H3PO4 to mols NaOH. That is mols H3PO4 x 3 = mols NaOH. Now M NaOH = mols NaOH/L NaOH. YOu know M and mols, solve for L NaOH and convert to mL.
Monday, December 10, 2012 at 8:06pm by DrBob222

chemistry- thank you
Write the equation. 2NaOH + H2SO4 ==> H2O + Na2SO4. moles H2SO4 = M x L = ?? moles NaOH needed = twice that (from the equation). Then M NaOH = moles NaOH/L NaOH. Solve for L NaOH.
Sunday, October 31, 2010 at 9:49pm by DrBob222

Chemistry DrBob
What is the pH of the solution created by combining 2.30 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 2.30 ________ _________ What are the pH values if you take into account that the 8.00 mL ...
Thursday, May 1, 2008 at 4:53pm by Amy

Chemistry-Is this correct?
The concentration of NaOH is normally in the range of 3-6 M when they peel potatoes and soak them in a solution of NaOH , remove them and spray them off. If I have 45.7 mL of 0.500M of H2SO4 required to react completely with a 20.0 mL sample of NaOh. What is the molar ...
Thursday, May 20, 2010 at 4:20pm by Sara

Chemistry
One commercial method used to peel potatoes is to soak them in a solution of NaOH for a short time, remove them from the NaOH, and spray off the peel. The concentration of NaOH is normally in the range of 3 to 6 M. The NaOH is analyzed periodically. In one such analysis, 45.7 ...
Wednesday, January 12, 2011 at 1:06am by Chin

chemistry
For the KHP question. Convert 0.51 g KHP to mols. mols = g/molar mass. You don't ask a question but I assume you want to know the molarity of the NaOH. Mols KHP = mols NaOH. mols NaOH = L x M. YOu have mols NaOH and L NaOH. Calculate molarity NaOH. Post yuor work if you get ...
Sunday, October 14, 2007 at 9:28pm by DrBob222

Chemisty
H2Ox + 2NaOH ==> Na2Ox + 2H2O mols Ox = grams/molar mass mols NaOH required = 2 x mols Ox (from th equation). M NaOH = mols NaOH/L NaOH/ Then to prepare 2.5L of solution you will need how many mols total? That is M x L = ? grams NaOH = mols NaOH/molar mass NaOH. You know ...
Wednesday, May 9, 2012 at 9:42am by DrBob222

Chemistry
Even if you can help answer one that would be a great help! 1. How many liters of NO(g) are produced when 0.85L of 2.00M HNO3 solution is added to 216g according to the equation. Which reactant is the limiting reactant? 3 Ag + 4 HNO3 -> 3 AgNO3 + NO + 2 H2O3 2. Calculate ...
Sunday, October 20, 2013 at 5:06pm by P.

Chemistry
So far so good; however, you didn't include the volume of NaOH required in the titration. M(NaOH) x mL(NaOH) = M(vinegar) x mL(vinegar). 0.1250 x mL(NaOH) = M(vinegar) x 4.00 mL Plug in the mL NaOH, whatever it is, and you will have just one unknown which is the molarity of ...
Wednesday, July 23, 2008 at 10:44pm by DrBob222

chemistry
How much 0.10 M Base (in mL) is required to neutralize 8.00 mL of the 0.10 M acid? Base Acid Base Volume (mL) NaOH HCl ___________ NaOH HC2H3O2 ___________ How would the volume of base change from problem above if the 8.00 mL of 0.10 M Acid was first diluted with 100 mL of ...
Thursday, May 1, 2008 at 12:42pm by Amy

chemistry
How much 0.10 M Base (in mL) is required to neutralize 8.00 mL of the 0.10 M acid? Base Acid Base Volume (ml) NaOH HCl ___________ NaOH HC2H3O2 ___________ How would the volume of base change from the problem above if the 8.00 mL of 0.10 M Acid was first diluted with 100 mL of...
Thursday, May 1, 2008 at 12:47pm by Amy

chemistry
KHP + NaOH ==> NaHP + H2O moles KHP = grams/molar mass Solve for moles. Look at the equation; it is 1:1 so moles KHP = moles NaOH.] The M NaOH = moles NaOH/L NaOH.
Saturday, October 16, 2010 at 12:26am by DrBob222

Chemistry help
There are numerous ways to do this but the shortest way is to use the dilution formula that you have in the last sentence of your post. I even take a short cut with that. 0.01M NaOH x (2.0 mL/8 mL) = ? M. Note: It isn't needed, but you really do have the mass. moles NaOH = M x...
Thursday, March 15, 2012 at 5:05pm by DrBob222

Chemistry
I will assume that this is a titration problem. You know the mass of the KHC8H4O4 (potssium hydrogen phthalate) and you titrated that mass with NaOH. mols phthalate = grams/molar mass. Since the equation is 1:1 (1 mol phthalate to 1 mol NaOH) the mols NaOH = mols phthalate ...
Sunday, October 7, 2012 at 12:21am by DrBob222

Chemistry
How many mols acetic acid did you use? That's M x L = ? Now use the equation coefficients to convert mols acetic acid to mols NaOH. That's a 1:1 ratio; therefore, mols NaOH = same as mols acetic acid. Then M NaOH = mols NaOH/L NaOH. You have mols and M NaOH, solve for L NaOH ...
Monday, May 13, 2013 at 5:11pm by DrBob222

chemistry
mols H2SO4 = M x L = ? mols NaOH = twice that (from the coefficients) M NaOH = mols NaOH/L NaOH. You know M and mols; solve for L and convert to mL. Click post answer
Wednesday, March 20, 2013 at 9:55pm by DrBob222

organic chemistry
First, this doesn't look like an organic chem question to me. I don't know any organic chemistry but this one I can work. moles NaOH = Molarity NaOH x liters NaOH = ? Convert moles NaOH to moles H2SO4 this way. ?mols NaOH x (1 mole H2SO4/2 moles NaOH = ?moles NaOH x 1/2 = x ...
Tuesday, January 31, 2012 at 10:01pm by DrBob222

Chem 100L
I worked this for someone last night. mols oxalic acid = grams/molar mass. Use the coefficients in the balanced equation to convert mols H2C2O4 to mols NaOH. M NaOH = mols NaOH/L NaOH
Sunday, December 2, 2012 at 3:40pm by DrBob222

Conductivity
Complete the table below: For each of the following sets pick the compound with the highest conductivity in a 1 M aqueous solution. (Enter the number at the top of the column containing the correct answer.) 1 2 3 Answers a HCl HC2H3O2 H2PO4 b KNO3 Ca(NO3)2 HNO3 c CH3OH NaOH ...
Wednesday, January 12, 2011 at 9:47pm by Helen

chemistry
KHP is a monoprotic acid with a molar mass of 204.22 g/mol. The titration data are as following. The average concentration of NaOH solution is M. 1 2 3 mass of KHP (g) 2.789 2.543 2.612 vol NaOH used (mL) 27.77 23.22 27.12 You didn't ask a question but I assume you are to ...
Wednesday, May 16, 2007 at 1:41am by jared

Chemistry
H2Ox + 2NaOH ==> 2H2O + Na2Ox moles H2Ox = grams/molar mass Convert moles H2Ox to moles NaOH using the coefficients in th balanced equation. That will give you moles NaOH = 2 x moles H2Ox. Then M NaOH = moles NaOH/L NaOH.
Saturday, March 26, 2011 at 11:39pm by DrBob222

chemistry
A volume of 100mL of 1.00 M HCl solution is titrated with 1.00 M NaOH solution. You added the following quantities of 1.00 M NaOH to the reaction flask. Classify the following conditions based on whether they are before the equivalence point, at the equivalence point, or after...
Monday, August 6, 2012 at 8:00pm by Anon

chem
Anytime the acid/base is the same; i.e., a monoprotic base(NaOH, KOH, NH3, etc) with a monoprotic acid (HCl, HC2H3O2, HBr, etc). It also is ok if they are both diprotic or triprotic. Diprotic acids are H2SO4, H2C2O4, etc) and diprotic bases are Ba(OH)2, Ca(OH)2, etc. The other...
Tuesday, October 30, 2012 at 6:26am by DrBob222

Chemistry
Aspirin, C9H8O4, is produced through the following reaction of salicylic acid, C7H6O3, and acetic anhydride, C4H6O3: C7H6O3(s) + C4H6O3(l) → C9H8O4(s) + HC2H3O2(l). a.) What mass of aspirin (in kg) could be produced from 75.0 mol of salicylic acid? b.) What mass of ...
Thursday, February 19, 2009 at 8:52pm by Emat

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