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April 21, 2014

Search: NaOH, HC2H3O2

Number of results: 4,889

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
Final buret reading = 31.10 Initial reading = 0 Volume NaOH = 31.10-0.0 = 31.10 mL. M NaOH = 0.2619M mols NaOH used = M x L = ? mols HC2H3O2 used = the same since this is a 1:1 reaction; i.e., NaOH + HC2H3O2 ==> NaC2H3O2 + H2O M HC2H3O2 = mols HC2H3O2/L HC2H3O2. You know L ...
Wednesday, March 20, 2013 at 3:58pm by DrBob222

Chemistry
Hi Dr. Bob, this is a chemistry question. I don't know how to go about solving this problem: What is the pH of the solution created by combining 11.40 mL of the 0.10 M NaOH(aq)with 8.00 mL of the 0.10 M HC2H3O2(aq)? Here's what I have so far: (0.10M NaOH)(0.0114L)= 0.00114 mol...
Wednesday, October 28, 2009 at 8:53pm by Yo

chemistry
HC2H3O2 + NaOH ==> NaC2H3O2 + H2O initial: HC2H3O2 = M x mL = 0.1 x 8.00 mL = 0.8 mmoles. NaOH = M x mL = 0.1 x 12.90 mL = 1.29 mmoles. NaC2H3O2 = 0 final: You have more NaOH than HC2H3O2; therefore, all of the HC2H3O2 will be used and some of the NaOH will remain. HC2H3O2...
Monday, May 3, 2010 at 2:00pm by DrBob222

chemistry
mols NaOH = M x L = ? mols HC2H3O2 = the same (note the balanced equation and 1 mol NaOH reacts with 1 mol HC2H3O2 which means 1:1). M HC2H3O2 = mols/L . YOu know mols and L.
Saturday, September 29, 2012 at 2:47pm by DrBob222

chemistry
Ka is ok. (HC2H3O2) is ok. Where is the (C2H3O2^-)? I don't see that anywhere. NaOH + HC2H3O2 ==> NaC2H3O2 + H2O Ka = (H^+)(C2H3O2^-)/(HC2H3O2) and solve for (H^+) = Ka*(HC2H3O2)/(C2H3O2^-) (H^+) = .... I get something like 4 x 10^-5 and pH about 4.4 or so. (You need to do ...
Monday, May 4, 2009 at 10:59am by rBob222

chemistry
Look at the equation. Base + acid = salt + water. NaOH + HC2H3O2 ==> NaC2H3O2 + H2O Calculate the moles NaOH to start. Calculate the moles HC2H3O2 to start. I haven't done the calculation but I assume that the HC2H3O2 will be in excess and all of the NaOH will be used. So ...
Monday, July 13, 2009 at 7:29pm by DrBob222

chemistry
What is the pH of the solution created by combining 2.40 mL of the 0.10 M NaOH(aq) with with 8.00 mL of the 0.10 M HC2H3O2(aq)? So, here's my working so far: .00024 mol NaOH .0008 mol HC2H3O2 .0008 - .00024 = .00056 mol HC2H3O2 .00056mol / 0.0104L = .05385 M HC2H3O2 The Ka of ...
Monday, May 4, 2009 at 10:59am by Brandon

Chemistry
What is the pH of the solution created by combining 12.20 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 w/HCl pH w/HC2H3O2 12.20 =================================== my work: 0.000420 moles of NaOH / 0.020 ...
Monday, May 3, 2010 at 2:50pm by Amphee

chem
What is the pH of the solution created by combining 2.40 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)? I understand how to find the pH for the NaOH + HCl solution. However, I'm not sure how to find it for HC2H3O2. I ...
Monday, May 2, 2011 at 8:10pm by Anonymous

Chem
This is a buffer solution disguised so it's a little harder to recognize. mols NaOH = L x M = 0.01130 x 0.100 M = ?? mols HCl = L x M = 0.00800 x 0.100 M = ?? Since the equation for the strong base and strong base is 1:1; i.e., NaOH + HCl ==> NaCl + H2O Just subtracting ...
Monday, October 29, 2007 at 4:00am by DrBob222

Chemistry DrBob
The NaOH + HCl part you know how to do from the previous problem I worked. And you are right about the volume of base not changing if the solution is diluted AFTER putting it in the titration vessel. For the NaOH + HC2H3O2 problem, you need to write the equation. It is NaOH + ...
Thursday, May 1, 2008 at 4:53pm by DrBob222

chemistry
STEP 1: STOICHIOMETRY to find moles C2H3O2- formed and HC2H3O2 remaining. All NaOH was used up, so that's how many moles reacted with the HC2H3O2 and also how many moles C2H3O2- formed. STEP 2: EQUILIBRIUM of HC2H3O2 with H+ and C2H3O2-. Change the moles of HC2H3O2 and C2H3O2...
Wednesday, April 29, 2009 at 9:18pm by Bill

chemistry
HC2H3O2 + NaOH ==> NaC2H3O2 + H2O How many moles is 1 g NaC2H3O2. That is g/molar mass = 1g/82 = 0.0122 moles. How can we get 0.0122 moles HC2H3O2. M = moles/L or L = moles/M = 0.0122/0.5 = 0.02440L or 24.40 mL of 0.5M HC2H3O2. Then dump in NaOH until all of it is ...
Wednesday, April 6, 2011 at 4:42pm by DrBob222

chemistry
There are two problems here. #1. pH when adding 1.90 mL of 0.1 M NaOH to 8.00 mL of 0.1 M HCl. moles NaOH = M x L = 0.0019 x 0.1 = 0.00019 moles moles HCl = 8.00 mL x 0.1 M = 0.008 x 0.1 = 0.0008. NaOH + HCl ==> NaCl + H2O Place the moles below the reactants so you can see ...
Sunday, July 11, 2010 at 8:46pm by DrBob222

Chemistry
Can a buffer solution with pH = 4.70 be prepared using water, 6.0 M HC2H3O2 and 6.0 M NaOH? Justify your answer. Ka = 1.8 x 10-5 for HC2H3O2 , K = 1.0 x 10-14 .
Wednesday, August 6, 2008 at 12:18am by Alexis

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
5% means 5.00g acetic acid in 100 mls of solution. That is equivalent to 50.0 g acid/L. The molar mass of acetic acid is about 60.05g/mole (50.0 g acid/L.)(1 mol / 60.05g) = 0.8326 mol/L The reaction is: HC2H3O2 + NaOH --> NaC2H3O2 + H2O based on the reaction, moles of ...
Thursday, October 22, 2009 at 10:18am by GK

chemistry
NaOH + HCl ==>NaCl + HOH Strong base + strong acid. calculate mols NaOH. M x L = ?? calculate mols HCl. M x L = ?? Determine mols NaCl and HOH produced. Determine excess NaOH OR HCl and pH from that. For NaOH + HC2H3O2 ==> NaC2H3O2 + HOH Strong base + weak acid. ...
Monday, May 5, 2008 at 5:31am by DrBob22

chemistry
You have two questions here. #1. pH of 0.8 mL x 0.1 M NaOH + 8.00 mL of 0.1 M HCl. moles NaOH = M x L = 0.1 x 0.0008 = 0.00008 moles NaOH. moles HCl = M x L = 0.1 x 0.008 = 0.0008 moles NaOH + HCl ==> NaCl + H2O Now place the moles under the reactants so you can see what is...
Monday, July 12, 2010 at 4:33am by DrBob222

chem-acid-base titrations
1/ HC2H3O2 + NaOH ==> HOH + NaC2H3O2 2. Calculate mols NaOH from L x M = ?? Convert mols NaOH to mols HC2H3O2 using the coefficients in the balanced equation. M acetic acid= mols/L. 3. Determine mols acetic acid in the 10 mL sample and from that grams acetic acid, then ...
Monday, April 21, 2008 at 10:06pm by DrBob222

Chemistry
How to solve titration problem for HC2H3O2 + NaOH= NaC2H3O2 + H2O The M of NaOH= 0.427 The volume of NaOH= 17.30mL 10.00mL of acid The second titration calculation is: The M of NaOH= 0.427 The volume of NaOH=34.60mL 20.00mL of acid
Thursday, September 27, 2012 at 8:16pm by John

chemistry
How to solve titration problem for HC2H3O2 + NaOH= NaC2H3O2 + H2O The M of NaOH= 0.427 The volume of NaOH= 17.30mL 10.00mL of acid The second titration calculation is: The M of NaOH= 0.427 The volume of NaOH=34.60mL 20.00mL of acid
Saturday, September 29, 2012 at 2:47pm by Anonymous

chem-acid-base titrations
ok for part 2 moles of NaOH=L*M .01*.5052=.005052 moles of NaOH then moles of NaOH =moles of HC2H3O2 since 1-1 ratio from equation that makes .005052 moles of HC2H3O2 correct? then M acetic acid=.005052 moles/.01688L which =2.9*10^-1 is that correct? and for part 3 is it mols ...
Monday, April 21, 2008 at 10:06pm by natash

Chem Webwork UCI
Complete the table below: What is the pH of the solution created by combining 0.70 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)? mL NaOH: 0.70 pH w/ HCl: 1.08 pH wHC2H3O2: 3.23 Complete the table below: What are the pH ...
Monday, April 25, 2011 at 4:50pm by Michelle

Chemistry
Hi, I posted yesterday with this lab question. "Calculate the molar amounts of NaOH used in the reaction with the HCl solution and with the HC2H3O2. I think I got the answer to that with the help that I received. I had 5 mL of HCl, and I was using .100 M NaOH, so I got 5x10-4 ...
Sunday, April 22, 2007 at 6:21pm by Rachel

Chemistry
If 25mL of 2.00M NAOH is added tpo 50mL of 0.10M HC2H3O2 (Ka=1.8*10^-5), what is the pH? moles HC2H3O2= c*v = .1 * .05L = .005 moles NaOH= c*v = .2 * .025L = .005 pH= Pka + log (B/A) = 4.75 + log (.005/.005) = 4.75 I'm not sure how to calculate the moles I know i'm making a ...
Monday, August 10, 2009 at 12:12pm by Sara

Chemistry
What is the pH of the solution created by combining 11.40 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)? Here is the chart that i am supposed fill out: mL NaOH pH w/ HCl pH w/ HC2H3O2 11.40 _________ ____________ Here's ...
Monday, April 27, 2009 at 7:32pm by Lisa

Chem
Remember this. acid + base = salt + H2O. I'll do the first one and leave the second for you. HCl + NaOH ==> NaCl + HOH. Just pull the H and OH out and what's left is the salt. HC2H3O2 + NaOH ==> On HC2H3O2, it's the FIRST H that is the acid H, the H3, for example, is ...
Tuesday, May 4, 2010 at 8:08pm by DrBob222

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

CHEMISTRY
How do you get the concentration with buret readings? What would the concentration of HC2H3O2 (M) be? For example, Molarity of the NaOH solution: 0.2619 M Final buret reading: 31.10 ml Initial buret reading: 0 Volume of NaOH solution: 31.0 ml concentration of HC2H3O2 (M...
Wednesday, March 20, 2013 at 3:58pm by Anna

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:12.30 pH w/ HCl _________ pH w/ HC2H3O2 _________ What are the pH values if you take into account that the 8....
Sunday, April 29, 2012 at 3:20am by HELP!!

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:12.30 pH w/ HCl _________ pH w/ HC2H3O2 _________ What are the pH values if you take into account that the 8....
Sunday, April 29, 2012 at 3:21am by HELP!!

Chemistry -- to Dr.Bob
I posted this yesterday and tried to work it out today but i don't remember how to. You said convert to moles by multiplying for example .1M x .008L= 8x10^-4 ...after this what do i do with this number to find the pH i tried to just plug that into the -log(8x10^-4) but it was ...
Friday, May 2, 2008 at 9:41pm by Amy

chemistry
What is the pH of the solution created by combining 11.40 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)? Complete the table below: Note: Make simplifying assumptions, do not use the quadratic formula. What are the pH ...
Sunday, October 30, 2011 at 9:10pm by Billy

chemistry desperately
i am completely lost, i confused myself. i need to find the concentration of HC2H3O2 HC2H3O2 + NaOH ==> NaC2H3O2 + HOH NaOH C= 0.3 M v= 0.25 L n= 0.075 moles M= 40.00g/mol m= 3.00 g NaC2H3O2 n= 0.075 moles m= 0.4973 g(ammount of acetic acid in solution) HC2H302 v= 0.020 L M...
Tuesday, December 16, 2008 at 12:10am by diana

Chemistry
Calculate the theoretical pH after 2.50 mL and 9.50 mL of NaOH has been added in both the titration of HCl and of HC2H3O2. Given: Molarity of all chemicals are 0.1 M HCl and HC2H3O2 are 8ml prepared in 100ml water.
Thursday, May 10, 2012 at 5:48pm by Raskin

CHEMISTRY (WEBWORK)
What is the pH of the solution created by combining 1.20 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 w/ HCl pH w/ HC2H3O2 1.20 ? ? Complete the table below: What are the pH values if you take into account ...
Monday, July 12, 2010 at 6:19pm by Anonymous

chemistry
Why does the equivalence point occur at different pH values for the four titration studied? the four titrations were: 1. HCL with NaOH 2.HC2H3O2 with NaOH 3. HCl with NH4OH 4. HC2H3O2 with NHOH Okay so equivalence point is when the number of moles of acids and bases are equal...
Friday, May 9, 2008 at 9:45pm by Amy

Chemistry DrBob
its two sorry the whole thing that i wrote didn't show up again. 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)? Here is the chart that i am supposed fill out: mL ...
Thursday, May 1, 2008 at 4:53pm by Amy

Chemistry
At 20 degrees celsius ,if the equation is C7H6O3(s)+C4H6O3(l)=C9H8O4+HC2H3O2(l), then how many liters of acetic acid, HC2H3O2 , would be formed if the density of HC2H3O2 is 1.05 g/ml?
Monday, February 6, 2012 at 11:49pm by Rene'

Chemistry 2 Lab
1.75 x 10^-5=Ka= {H3O}{C2H3O2)/{HC2H3O2} lets do the first one, HC2H3O2 + H2O----> H3O+ + C2H3O2- pH=3, so H3O+=10^-(3)=1 x 10 ^-3 M so the ratio of H3O+= C2H3O2- So, Ka=1.75 x 10^-5= {H3O}{C2H3O2)/{HC2H3O2} becomes Ka=1.75 x 10^-5= [1 x 10 ^-3 M][1 x 10 ^-3 M]/{HC2H3O2}, ...
Tuesday, March 19, 2013 at 6:50pm by Devron

chemistry
Two questions. The point of these two problems is to show the difference between neutralizing a strong base with a strong acid versus neutralizing NaOH (a strong base) with a weak acid (HC2H3O2). NaOH + HCl ==> NaCl + HOH So you look to see what you have when mixing these ...
Wednesday, July 9, 2008 at 12:19am 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
correction: the base is NaOH and acid is HC2H3O2
Wednesday, April 9, 2008 at 2:08am by tia

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
Yes, the pH is 7. I made that post and I hit the wrong key. Of course 7.0 is the correct answer and not 8 for NaCl. For the other part, if you exactly neutralize NaOH and acetic acid, you will have at the equivalence point a solution of sodium acetate, the salt of a weak acid ...
Monday, July 12, 2010 at 3:05am by DrBob222

chemistry
Calculate the theoretical pH after 2.50 mL and 9.50 mL of NaOH has been added in both the titration of HCl and of HC2H3O2. Indicate if the volume of NaOH is before or after the equivalence point.
Friday, May 9, 2008 at 9:45pm by paige

chem lab
Calculate the theoretical pH after 2.50 mL and 9.50 mL of NaOH has been added in both the titration of HCl and of HC2H3O2. Indicate if the volume of NaOH is before or after the equivalence point. i dont know where to start.
Tuesday, May 10, 2011 at 2:00am by Anonymous

Chemistry
To make things a little easier to type, let's realize that CH3COOH (acetic acid and written HC2H3O2) can be called HAc where H is the terminal H of the COOH and Ac stands for the remainder of the molecule. NaOH + HAc ==> NaAc + H2O moles NaOH you have. 0.1 M x 0.01140 = 0....
Wednesday, October 28, 2009 at 8:53pm by DrBob222

chemistry
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 pH with HCl pH with HC2H3O2 1.90 ? ?
Sunday, July 11, 2010 at 8:46pm by Sara

chemistry
REVISION TO PREVIOUS POST: 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)? I understood how to do the HC2H3O2, but I can't do the HCl. I am trying to do the same ...
Sunday, July 11, 2010 at 10:08pm by Sara

chemistry
how many mL of 1M HC2H3O2 are required to neutralize a spill of 25mL of 6M NaOH?
Tuesday, December 7, 2010 at 12:23am by erin

chemistry
which solution has the lower pH? a)0.1 M HCL or 0.1 M HC2H3O2? b)0.1 M NaOH or 0.1 M NH3? c)0.1 M Na2CO3 or 0.1 M NaCl?
Wednesday, November 9, 2011 at 2:45am by denis

chemistry
balanced equation: HC2H3O2 + NaOH -> What is the mole ratio of these two substances?
Tuesday, November 29, 2011 at 4:47pm by science

Chemistry
What is the pH of the solution created by combining 12.40 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)? I know how to solve for HCl but not with HC2H3O2.
Saturday, May 1, 2010 at 8:43pm by Manali

Chemistry
Subjects Art Business Computers English Foreign Languages Health Home Economics Mathematics Music Physical Education Science Social Studies Features Contribute Download Experts Forum Job Openings Homework Tips Libraries.Jiskha Link to Us Reference School Supplies Search ...
Monday, July 9, 2007 at 1:12pm by Jared

chemistry
I'll let HAc stand for HC2H3O2. Then NaOH + HAc ==> NaAc + H2O. Calculate mols NaOH. mols = L x M = ?? Calculate mols HAc. mol = L x M = ?? They react in 1:1 ratio. Use logic to determine how much NaAc is produced and how much NaOH remains unreacted. Note: Check the problem...
Wednesday, April 9, 2008 at 2:08am by DrBob222

Chemistry Titration Lab
Calculate the theoretical pH after 2.50 mL and 9.50 mL of NaOH has been added in both the titration of HCl and of HC2H3O2. Given: Molarity of all chemicals are 0.1 M HCl and HC2H3O2 are 8ml prepared in 100ml water. Im guessing I need to make and ICE chart but I'm having ...
Thursday, May 5, 2011 at 11:07pm by Kim

Chemistry
You need to learn to do these. The easy way, in the beginning, is to write the hydrolysis as if the salt (all of them) reacted completely with water, then apply rules to know what happens. For example, for NaC2H3O2, NaC2H3O2 + HOH ==> NaOH + HC2H3O2. That is step 1. Step 2...
Saturday, April 30, 2011 at 6:52pm by DrBob222

CHEMISTRY
which of the following represent a buffer system? A.) NaOH and NaBr B.) HF and NaF C.) HC2H3O2 and C12H22O11 D.) HCl and KOH
Saturday, March 3, 2012 at 8:39pm by dylan

chem urgent!!
What is the pH of the solution created by combining 12.00 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)? i need to find the ph with HCL and then with hc2h3o2. i got 1.30 as my anser but this was wrong i multipled all these...
Wednesday, August 20, 2008 at 7:57pm by tom

chem lab (webwork)
Complete the table below: 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
Tuesday, April 13, 2010 at 7:19pm by need help student

Chemistry
Commercial vinegar was titrated with NaOH solution to determine the content of acetic acid, HC2H3O2. For 20.0 milliliters of the vinegar 26.7 milliliters of 0.600-molar NaOH solution was required. What was the concentration of acetic acid in the vinegar if no other acid was ...
Wednesday, May 23, 2007 at 11:38pm by Sarah

11th grade CHEMISTRY TITRATION LAB!
I am somewhat confused but I can answer most of your questions. Vinegar is acetic acid and you are doing th titration in order to determine the concentration of acetic acid in vinegar. Acetic acid is HC2H3O2 and the first H on the left in the formula is the acidic hydrogen (...
Sunday, December 14, 2008 at 8:56pm by DrBob222

General Chemistry
Calculate the theoretical pH after 2.50 mL and 9.50 mL of NaOH has been added in both the titration of HCl and of HC2H3O2. Indicate if the volume of NaOH is before or after the equivalence point. Compare these theoretical values with the actual values found on the titration ...
Sunday, November 6, 2011 at 9:28pm by Ashley

Chemisty (please read soon)
which will become a buffer in 1L of H2O? a) 0.3 mole KOH & 0.3 mole HBr b) 0.5 mole NH3 & 0.5 mole HCl c) 0.2 mole NaCl & 0.3 mole HCl d) 0.2 mole NaOH & 0.2 mole HBr e) 0.4 mole HC2H3O2 & 0.2 mole NaOH I think that the answer is e. Is that correct?
Sunday, April 29, 2012 at 11:03pm by Zac

Chem Webwork help
1. What is the pH when enough 0.10 M Base (in mL) is added to neutralize 8 mL of 0.10 M Acid? Complete the following table. NaOH HC2H3O2 2. What is the pH of the solution created by combining 2.60 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of ...
Monday, July 12, 2010 at 2:34am by Sammy

chem lab (webwork)
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
Tuesday, April 13, 2010 at 7:20pm by anonymous

AP Chemistry
In a titration of 50 mL 1 Molar HC2H3O2 with 1 Molar NaOH, a student used bromcresol green as an indicator (Ka = 1 X 10^-5). About how many mL of NaOH would it take to reach the end point with this indicator? What would be a better indicator for this titration; why?
Saturday, April 3, 2010 at 7:07pm by Jessica

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
If it requires 30.0 milliliters of 1.2 molar HCl to neutralize 20.0 milliliters of NaOH, what is the concentration of the NaOH solution? Balanced equation: NaOH + HCl NaCl + H2O 0.60 M NaOH 0.80 M NaOH 1.3 M NaOH 1.8 M NaOH
Wednesday, June 22, 2011 at 12:14pm by Magan

chemistry
What is the pH when enough 0.10 M Base NaOh (in mL) is added to neutralize 8 mL of 0.10 M Acid HCl? Acid HC2H3O2? I got the pH of HCl to be 7 because I figured that the same molarity of base and acid are added together to neutralize the pH, but I keep messing up for HC2H3O2. I...
Sunday, July 11, 2010 at 11:12pm by Sara

Chemistry 1115
What is the chemical equation for the reaction that occurs when you add 0.1 M NaOH solution to the HC2H3O2-NaC2H3O2 buffer solution?
Sunday, November 25, 2012 at 8:03pm by Marci

AP Chemistry
What volume of each of the following acids will react completely with 25.50 mL of 0.700 M NaOH? (a) 0.100 M HCl (b) 0.150 M HNO3 (c) 0.200 M HC2H3O2
Saturday, September 24, 2011 at 9:13pm by Rahul

Chemistry
Calculate the theoretical pH after 2.50ml and 9.50ml of NaOH has been added in both the titration of HCl and of HC2H3O2.
Tuesday, May 10, 2011 at 4:47pm by anna

Chemistry
2. Calculate the mass of water produced when 0.333L of 0.500M NaOH is added to 3.0g of acetic acid. The equation is: NaOH + HC2H3O2 -> NaC2H3O2 + H2O This is another LR problem. The only difference is that the end product is to convert mols to grams instead of volume as in ...
Sunday, October 20, 2013 at 5:06pm by DrBob222

chemistry
If 36.3 ml of 0.152M NaOH is required to neutralize 25.00 ml of an HC2H3O2 solution ,what is the molarity of the acetic acid?
Tuesday, September 11, 2012 at 10:44pm by HJ

Chem
(Na^+) = (NaOH) mols NaOH = M x L (NaOH) = (M NaOH x L NaOH/total volume) = 0.200 x 0.100/0.350) =? The others look ok to me.
Monday, October 28, 2013 at 10:14pm by DrBob222

Chemistry
Ok, I think I have this one but can you please check my work? A nationally known company markets a product called "cleaning vinegar" that is not designed for human consumption. What is the Mass Percent of acetic acid (HC2H3O2) in this product, if 25 drops of .683 M NaOH ...
Monday, March 5, 2007 at 11:16pm by Toni HELP!

chemistry
how do you make 1.00g of NaC2H3O2 using: 0.400 M Na2Co3 0.300 M Pb(C2H3O2)2 NaOH solution with unknown molarity 0.500 M HC2H3O2 You dont have to use all of them
Wednesday, April 6, 2011 at 4:42pm by stephanie

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....
Thursday, April 15, 2010 at 11:05pm by anonymous

chem
I got part 1: What is the pH of the solution created by combining 1.10 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)? pH w/HCl =1.12 w/HC2H3O2(aq)= 3.94 But how do you do part two? What are the pH values if you take into ...
Thursday, April 29, 2010 at 12:13am by Adam

Chemistry
my ap chem teacher has been absent for the past two weeks and part of the notes her sub gave us to copy says that In the equation HC2H3O2 + H20 <--> C2H3O2(- charge) + H3O(+ charge) HC2H3O2 is an acid H2O is a base C2H3O2(- charge) is the conjugate base and H3O(+ charge...
Saturday, May 15, 2010 at 3:51pm by Mark

Chemistry
The equilibrium in both mixtures is: HC2H3O2(aq) <=> H+(aq) + C2H3O2^-(aq) For the first mixture use the Henderson-Hasselbalch Equation to get the pH: pH = pKa + log{[C2H3O2^-]/[HC2H3O2]} NOTE: [C2H3O2^-] = molarity of NaC2H3O2 pH = pKa + log{1} In the second mixture, ...
Thursday, July 16, 2009 at 3:36am by GK

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
The technical way of saying it is that if the anion is a stronger base than water, then the solution will be basic. If the cation is a stronger acid than water, then the solution will be acid. If the cation and anion are equally strong, the solution will be neutral. ...
Monday, March 16, 2009 at 9:21pm by DrBob222

Chemistry
What is the pH of the solution created by combining 2.70 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)? 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...
Monday, May 3, 2010 at 3:37pm by Ashley

Chemistry
What is the pH of the solution created by combining 2.70 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)? 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...
Monday, May 3, 2010 at 3:37pm by Ashley

Chemistry
Household vinegar is aquous, 5% acetic acid HC2H3O2 solution by mass. The molarity is: 5% = 5g 1mol HC2H3O2 = 60.05g HC2H3O2 5g/60.05g = 0.08326394671 mol therefore the molarity is 0.08326394671 mol/0.01L = 0.84mol/L
Sunday, April 10, 2011 at 10:26pm by Ntswaki Ramalobela

Chem 1A
Help please! How many moles of NaOH must be added to 1.0 L of 3.0 M HC2H3O2 to produce a solution buffered at each pH? 1) pH= 3.78 2) PH= 6.52
Thursday, March 15, 2012 at 10:01pm by Mackenzie

CHEM 101
HBr + NaOH ==> NaBr + H2O mols HBr = M x L = ? Convert mols HBr to mols NaOH using the coefficients in the balanced equation. M NaOH = mols NaOH?L NaOH. You have M NaOH and mols NaOH, substitute and solve for L NaOH (and convert to mL if that is needed).
Tuesday, October 8, 2013 at 11:39am by DrBob222

chemistry
how do you solve this What is the pH of the solution created by combining 2.60 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 2.60 pH wHCl: _ pH wHC2H3O2 : _ Complete the table below: What are the pH values if you ...
Monday, July 12, 2010 at 6:03pm by Jin

chemistry
What is the pH of the solution created by combining 12.90 mL of the 0.10 M NaOH with 8.00 mL of the 0.10 M HC2H3O2?
Monday, May 3, 2010 at 2:00pm by jc

chemistry
Calculate the pH of a solution prepared by mixing 25.0 mL of 0.60 M HC2H3O2 and 15.0 mL of 0.60 M NaOH?
Thursday, May 6, 2010 at 3:58pm by Julie

Chemistry
How much 0.10 M NaOH (in mL) is required to neutralize 8.00 mL of the 0.10 M HC2H3O2?
Sunday, May 2, 2010 at 12:57pm by John

pH- part 2
how much .10M Base (in mL) is needed to neutralize 8.00mL of .10M Acid? base- NaOH, acid- HCl, base volume (mL)- ? base- NaOH, acid- HC2H3O2, base volume (mL)- ? VaNa=VbNb Vb= 8ml*.10N/.10N= 8m.
Saturday, April 14, 2007 at 6:27pm by Christine

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
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

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

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