Search: titrated

Number of results: 784

chemistry
Determine the volume of the titrant that would effect of neutralization. a.)0.036 L OF 0.98 m HCL titrated with with 0.58 NaOH b.) 24.3 mL of 0.29 M H2SO4 titrated with 0.42 M KOH
Sunday, October 9, 2011 at 8:30pm by Anonymous

Chem Will somebody Please help me
Yes, most are titration erxperiment but in some cases the tablet is titrated directly; in others the tablet is dropped into a set volume of acid, then the excess acid is back titrated with standard base so that the amount of acid used is the difference between the initial ...
Wednesday, February 20, 2013 at 10:34pm by DrBob222

Chemistry
The indicator used was Eriochrome Black T, and for the double titration... I don't know. I know that NaOH was added to precipitate Mg(OH)2, and then it was titrated with EDTA. Then it was left to sit for 5 minutes to dissolve any precipitated Ca(OH)2, and titrated again to...
Sunday, March 14, 2010 at 10:53pm by Johnathan

Chem
mols potassium hydrogen tartrate = grams/molar mass = 0.12/molar mass = ? You took 10/25 of this for titration; therefore, mols titrated = mols initially x 10/25 = ? M NaOH = mols tartrate titrated/L NaOH. You know M NaOH and mols titrated, solve for L NaOH and convert to mL.
Friday, March 8, 2013 at 8:44pm by DrBob222

Analytical Chemistry
You have the mass of the KHP sample. You weighed out 0.5050 g (of course you've diluted it; perhaps that is the question; i.e., what is the mass of the KHP in the titrated sample? :-). How many moles NaOH did you use? M x L = moles = 0.0067M x 0.01475 = 9.88E-5 moles NaOH...
Wednesday, July 20, 2011 at 10:38am by DrBob222

Chemistry
You titrated to the CO3^2- end point so the equation chemistry is what I indicated. I've never used that indicator. I always used methyl red and titrated until the indicator turned, heated to drive off CO2 (the m.r. turned back basic, and I titrated to the end point (much ...
Sunday, October 21, 2012 at 9:35pm by DrBob222

chem
OK EXCEPT that the mass is not 7.5 grams. You titrated only 25 mL aliquot of the original sample of 250 mL; therefore, you titrated only 0.75 g. Thus 0.75/5.55 x 10^-3 = ?? molar mass
Saturday, July 24, 2010 at 2:18pm by DrBob222

Chemistry
Calculate the pH at the halfway point and at the equivalence point for each of the following titrations. (a) 100.0 mL of 0.14 M HC7H5O2 (Ka= 6.4 multiplied by 10-5) titrated by 0.14 M NaOH halfway point equivalence point (b) 100.0 mL of 0.29 M C2H5NH2 (Kb = 5.6 multiplied by ...
Friday, June 1, 2012 at 5:13pm by Andrew

Chemistry
Hi Can someone please help me undersand how to get the answer to this question A 15.0 mL solution of 0.050 mol/L AgNO3 was titrated with 0.0250 mol/L NaBr in the cell SCE || titrated solution | Ag(s) Find the cell voltage for 10.0 mL of titrant added. (a) -0.0312 V (b) 0.194 V...
Monday, April 26, 2010 at 6:53am by James

Chem 2
Checking to see if I did this right? Titration of HN03 titrated with NaOH ending result is 1.38. Titration A, endpoint pH = 8 is pKa or pKb= 1.38x106=5.861 and Titration of NH03 titrated with KOH ending results 1.54. Titration B, endpoint pH = 7 is KaorKb= Ka=1.54x105
Wednesday, March 21, 2012 at 11:58pm by Debbie

CHEMISTRY: URGENT DRBob222
Why was the reaction mixture titrated quickly? (question fom: A mixture of 0.50 mol of ethanoic acid and 1.00 mol of ethanol was shaken for a long time to reach equilibrium. The whole mixture was titrated quickly with 1.00 mol dm3 sodium hydroxide and 80cm3 of alkali were ...
Thursday, March 14, 2013 at 8:45pm by LC-Laila

science
I would use precision instead of accuracy in #1. #2 I don't understand. It seems to me that how fast you stirred is not relevant as long as you stirred it so as to mix completely. Rewording to that context would make more sense to me. For #3, you may have made an error in ...
Saturday, January 12, 2008 at 12:34pm by DrBob222

chemistry
In a similar experiment to yours, one tablet of Antacid A is titrated to its endpoint with 15.5 mL of 0.5 M HCl and one tablet of Antacid B is titrated to its endpoint with 24.3 mL of 0.5 M HCl. Which is the more effective antacid?
Wednesday, December 7, 2011 at 7:34pm by Anonymous

College Chemistry
"A student weighs 0.347 g of KHP on a laboratory balance. The KHP was titrated with NaOH and the concentration of the NaOH determined to be 0.110 M. For the second titration, the student correctly diluted 6 M HCl from the reagent shelf using a graduated cylinder to obtain...
Wednesday, October 20, 2010 at 10:49am by James

Chemistry
The Question Is: "A student weighs 0.347 g of KHP on a laboratory balance. The KHP was titrated with NaOH and the concentration of the NaOH determined to be 0.110 M. For the second titration, the student correctly diluted 6 M HCl from the reagent shelf using a graduated ...
Wednesday, October 20, 2010 at 1:48am by James

College Chemistry
The Question Is: "A student weighs 0.347 g of KHP on a laboratory balance. The KHP was titrated with NaOH and the concentration of the NaOH determined to be 0.110 M. For the second titration, the student correctly diluted 6 M HCl from the reagent shelf using a graduated ...
Tuesday, October 19, 2010 at 11:10pm by James

chemistry
1) a 100ml smaple of 0.18M HCLO4 is titrated with 0.27M LiOH. determine the ph of the soution after the addition of 66.67 ml of LiOH (this is at equivalence point) 2)a 100 ml sample of .20M HF is titrated with .10M KOH. determine th ph of the soution before the addition of any...
Tuesday, March 8, 2011 at 2:26am by lia

Chem
moles NaOH = M x L. moles weak acid = moles NaOH IF the weak acid is a monoprotic acid; otherwise, moles acid will be 1/2 if diprotic (and both hydrogens are titrated together) or 1/3 if triprotic (and all three hydrogens are titrated together).
Sunday, October 3, 2010 at 12:19am by DrBob222

Chemistry
How do I do this problem? 1. A student did an alkalinity determination correctly, except that the sample titrated had a volume of 90.0 mL. Volume A was found to be 4.50 mL and Volume B was 7.00 mL. a) Calculate the alkalinity value from these data and then calculate the ...
Tuesday, March 13, 2007 at 10:36pm by Joe

Chemistry
If I didn't make an error, you and I differ by a factor of 100. Did you correct the titrated amount to the original solution by multiplying by 100? 1. mols I2 = M x L = 0.00660 x 8.5E-4 [= 5.61E-6 mols vit C in titrated sample. 2. 5.61E-6 x (100/1) = 5.61E-4 moles in the ...
Monday, March 12, 2012 at 8:26pm by DrBob222

Chemistry
Redox titrations are used to determine the amounts of oxidizing and reducing agents in solution. For example, a solution of hydrogen peroxide, , can be titrated against a solution of potassium permanganate, . The following equation represents the reaction: 2KMnO4+H202-&gt...
Saturday, September 18, 2010 at 8:12pm by Peter

Chemistry
You started in the middle of the question. I'm just guessing that you have performed an experiment in which you determined %Cu in a sample. The equations are Cu^2+ + KI(xs) ==> CuI(s) + I2 and I suppose you titrated the liberated I2 with thiosulfate like this 2S2O3^...
Sunday, February 26, 2012 at 4:06pm by DrBob222

Chem
Ores are analyzed by dissolving some of the ore and then performing an analysis of a metal (expressed in grams); usually the concentration of the metal is expressed as % of the amount of the ore (in grams) dissolved. An ore containing V was dissolved and then titrated with ...
Sunday, April 7, 2013 at 1:13am by Mariam

chemistry
Topic: Iodometry 1. the reason why the Cu2+ solution has to be titrated immediately after addition of KI - I thought, because if allowed to stand for a long time, iodine will volatilize and a change in concentration of iodine will occur...is this right? Please correct me if I...
Sunday, July 29, 2007 at 11:54am by smiley

chemistry repost
Alex--Is there any/some indication of the end point to which the NaOH/Na2CO3 was titrated? My point is that Na2CO3 to the phenolphthalein end point (about pH 9) titrates to NaHCO3 whereas Na2CO3 titrated to the methyl red or methyl orange end point (about pH 4 or 5) titrates ...
Monday, April 21, 2008 at 9:38pm by DrBob222

Chemistry
Yes to the ICE table (at least a modified one) and no, there is no limiting reagent. First you want to determine the moles HCl and moles H3PO4 mixed. M x L = moles. All of that is added to a 1 L volumetric flask, diluted to the mark. So what is the concn of HCl and H3PO4. ...
Sunday, April 19, 2009 at 5:22pm by DrBob222

Chemistry
Calculate the final concentration for the standardization of KMnO4 given this information: 2MnO4- + 5C2O4^-2 + 16H+ -> 2Mn^2+ + 10CO2 + 8H2O [final redox equation] Volume of KMnO4 titrated with H2SO4 + Na2C2O4 = 293 mL Volume KMnO4 titrated with H2SO4 alone = 0.2 mL ...
Wednesday, May 2, 2012 at 1:15pm by Katherine

chemistry
H2A + 2NaOH ==> 2H2O + Na2A The rest of what is titrated? I'm assuming you titrated all of it. mols NaOH = M x L mols acid = 1/2 mols of NaOH (look at the coefficients in the balanced equation). mols acid = grams/molar mass. You know mols and grams, solve for molar ...
Tuesday, October 23, 2012 at 2:42pm by DrBob222

Chemistry
A 25.0cm^3 aliquot of a solution containing Fe2+ ions and Fe3+ ions was acidified and titrated against KMnO4 solution. 15.0cm^3 of 0.020M KMnO4 was needed. A second 25.0cm^3 aliquot was reduced using Zn, then titrated. This time, 19.0cm^3 of the 0.020M KMnO4 was needed. ...
Wednesday, March 9, 2011 at 11:27pm by tam

analytical chemistry
mL used = 25.01-12.38 = 12.63 mL of 0.0252M HCl. mols HCl = 0.0252 x 0.01238 = about 0.00031 (but you need to be more careful with these numbers) You titrated 50 mL of the diluted NaOH; therefore, the M of the titrated solution is 0.00031/0.050L = about 0.0062M That solution ...
Thursday, February 21, 2013 at 2:16pm by DrBob222

Chemistry
You don't say to which end point the triprotic acid was titrated. It could be titrated to the first H, the second, or all three. I will assume all three H ions were neutralized. H3A + 3KOH ==> K3A + 3H2O moles KOH = M x L = ?? Using the coefficients in the balanced ...
Saturday, March 26, 2011 at 9:37pm by DrBob222

Chemistry
It's important to know what you used as an indicator. If you used phenolphthalein you titrated to the HCO3^- end point. If you used methyl orange or methyl red you titrated to the H2CO3 (H2O + CO2) end point. I will assume that's the one you used.(I think M.R. is ...
Sunday, October 21, 2012 at 9:35pm by DrBob222

College Chemistry
1) A 25mL sample of the .265M HCI solution from the previous question is titrated with a solution of NaOH. 28.25mL of the NaOH solution is required to titrate the HCl. Calculate the molarity of the NaOH solution. 2) A 1.12g sample of an unknown monoprotic acid is titrated with...
Monday, October 25, 2010 at 2:29pm by Jessica

chemistry
1gm of AgNO3 is dissolved in 50ml of h2o. it is titrated with 50ml od sol. agi is precipitated is filtered of.the exces of ki is then titrated with 1/10M KIO3 in the presence of acidic medium until all I->>ICl. it reqires 50ml of the 1/10M KIO3 sol. 20ml of same ...
Sunday, March 28, 2010 at 12:55am by debby

Chemistry
Redox titrations are used to determine the amounts of oxidizing and reducing agents in solution. For example, a solution of hydrogen peroxide,H2O2, can be titrated against a solution of potassium permanganate, KMnO4. The following equation represents the reaction: 2KMnO4(aq)+...
Sunday, October 3, 2010 at 4:29pm by Ellen

college
How do i calculate the number of equivalents of h2c4h4o4 titrated?
Wednesday, October 20, 2010 at 12:36pm by Kaitlyn

chemistry
Actually you have several questions rolled into one. The simplest answer is that CO2 is absorbed by the NaOH and that decreases the molarity of the standard base. IF the indicator is one that changes in the acid region (for example, bromocresol green or methyl red) then no ...
Sunday, January 18, 2009 at 11:08pm by DrBob222

CHEMISTRY
1) An NaOH solution of unknown concentration is titrated with HCl. 51.9 mL of 0.400 mol/L HCl will neutralize 75.0 mL of the NaOH. What is the concentration of the NaOH solution ? Record your answer in decimal notation. I think the answer is 0.277 mol/L. is that right? 2)An ...
Tuesday, January 31, 2012 at 9:17pm by TIANDRA

chemistry
Sorry i guess i missed some. It is titrated with HCl
Monday, September 20, 2010 at 11:08pm by Heather

Chemistry
A couple of points. If HCl is the titrant, your statement should be "a sample of NaOH is titrated with HCl" and if you do it that way you do not need the statement that HCl is the titrant. Second point is that the problem doesn't make it clear how much HCl was ...
Thursday, February 24, 2011 at 1:13pm by DrBob222

chemistry
From the balanced equation for tums and .0072mL calculate no. moles titrated.
Thursday, February 9, 2012 at 4:37pm by Everett

chemistry/stiochiometry
does it make a difference if the base was titrated because i forgot to mention that
Wednesday, March 16, 2011 at 9:41pm by Anonymous

GChem
1. 25mL of 0.1M HCl is titrated with 0.1M NaOH. What is the pH when 30mL of NaOH have been added? 2. 25mL of 0.1M HCl is titrated with 0.1M NaOH. What is the pH after 15mL of NaOH have been added? I don't know how to make calculation I assumed that for number 1 when you ...
Monday, August 10, 2009 at 12:20pm by Mike

Chemistry (Titration Curves)
And btw, bases are being titrated into acids.
Sunday, May 8, 2011 at 12:44am by Anonymous

CHEM
0.16 M HC2H3O2 and 0.31 M of NAC2H3O2 titrated with what ml of 0.25 M HCL
Thursday, March 24, 2011 at 6:48am by bID

ap chemistry
I want to make a couple of points here. 1. The equation provided by GK works quite well for both of these problems; however, it is good ONLY for those equations in which the mol ratios of acid to base is 1 as they are in HCl and NaOH. If H2SO4 was being titrated with NaOH it ...
Thursday, October 2, 2008 at 10:19pm by DrBob222

chemistry
Draw the titration curve of H2C6H6O6 (ascorbic acid, diprotic) titrated with NaOH.
Wednesday, March 14, 2012 at 3:34am by Bailey

CHEM
You need to know the volume of the solution being titrated. Are the two solutions mixed (buffer)?
Thursday, March 24, 2011 at 6:48am by Liz

science(chem)
I need help finding information on how the conway microdiffusion is done/how it works. And why the sample is titrated. Thank you
Saturday, September 13, 2008 at 11:09pm by ~christina~

science(chem)
I need help finding information on how the conway microdiffusion is done/how it works. And why the sample is titrated. Thank you
Friday, September 12, 2008 at 11:05am by ~christina~

chemistry
what are the reasons why the Cu(II) solution has to be titrated immediately after addition of KI?
Thursday, January 31, 2008 at 11:41am by irma

Chemistry
You took a 25.00 mL sample and diluted t 250.0 mL and titrated a 50.00 mL aliquot. You have the weight in the 50.00 mL sample. The weight in the original 25.00 mL sample is weight in titrated sample x (250/50) = ? Now you have the weight in the original 35.00 mL sample and ...
Wednesday, March 28, 2012 at 5:26am by DrBob222

chemistry
from Balanced CaCO3+2HCL-CaCL2+H2O+CO2 and 7.2*10^-3 L Calculate moles titrated
Thursday, February 9, 2012 at 6:28pm by Everett

chemistry/stiochiometry
the acid is titrated against the base i might have said that wrong last time
Wednesday, March 16, 2011 at 9:41pm by Anonymous

acid and base titrations
You want to use a titrant that is close to that of the sample being titrated so I would choose a.
Sunday, November 21, 2010 at 5:15am by DrBob222

chemistry
50.00 mL of OOH was diluted to 250.0 mL with deionized water. In the determination of the total cation concentration, 25.00 mL aliquots of the dilute OOH were passed through a cation exchange column and the eluent titrated with an average 27.42 mL of 0.1134 M NaOH. In the ...
Thursday, January 26, 2012 at 10:17pm by Annabelle

Chemistry
50.00 mL of OOH was diluted to 250.0 mL with deionized water. In the determination of the total cation concentration, 25.00 mL aliquots of the dilute OOH were passed through a cation exchange column and the eluent titrated with an average 27.42 mL of 0.1134 M NaOH. In the ...
Thursday, January 26, 2012 at 5:51am by Georgia

Chemistry
HOBr (aq) <----> H+ (aq) + OBr- (aq), Ka = 2.3 x 10^-9 Hypobromous acid, HOBr, is a weak acid that dissociates in water, as represented by the equation. (a) Calculate the value of [H+] in a solution of HOBr that has a pH of 4.95. Ans: 1.1 * 10^-5 M (b) Write the ...
Tuesday, April 10, 2012 at 7:22pm by Confused

Chemistry
This problem is one of misdirection. You can ignore everything at the beginning and start with "A sample of ......" mols KOH used = 0.0255 x 1M = 0.0255 mols CH3COOH titrated = 0.0255 = mols CH3COOK formed at the equivalence point. (CH3COOK) = 0.0255 mols/total ...
Tuesday, May 1, 2012 at 11:18am by DrBob222

science
How would your results have differed if you had over-titrated, i.e. added NaOH beyond the endpoint?
Monday, November 12, 2012 at 7:45pm by nicki

chemistry
how many moles of acetic acid are in 15.05mL, 45.13mL, and 75.22mL of titrated vinegar?
Friday, May 14, 2010 at 10:39am by nik

CHEMISTRY: URGENT DRBob222
A mixture of 0.50 mol of ethanoic acid and 1.00 mol of ethanol was shaken for a long time to reach equilibrium. The whole mixture was titrated quickly with 1.00 mol dm3 sodium hydroxide and 80cm3 of alkali were required. 1. Write an equation for the reaction between ethanoic ...
Thursday, March 14, 2013 at 5:54pm by LC-Laila

Chemisttry
A 100.0-mL sample of 0.250 M aniline (C6H5NH2) is titrated with 0.500 M HCl. What is the pH at the equivalence point?
Sunday, May 6, 2012 at 4:36pm by Jake

AP Chem
Consider 25.0 ml of .300 MHNO2 that is titrated with .500 M Find ph at eq pt
Monday, April 23, 2012 at 5:49pm by Anna

chemistry
Topic: Iodometry 1. the reason why the Cu2+ solution has to be titrated immediately after addition of KI Answered above.
Sunday, July 29, 2007 at 11:49am by smiley

chemistry
The idea here is that an excess of HBr was added to Ba(OH)2. Some reacted with Ba(OH)2 and some was left over. How much was left over? That amount is what was titrated with the NaOH. Ba(OH)2 + 2HBr ==> 2H2O + BaBr2 +(xs HBr) mmoles HBr initially = 400.0 x 0.5000M = 200....
Saturday, February 26, 2011 at 2:38pm by DrBob222

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

chemistry
A sample of ammonia (Kb = 1.8 * 10-5) is titrated with 0.1 M H2SO4. At the equivalence point, the pH is approximately Isn't it should be 5 right i believe.
Tuesday, May 18, 2010 at 4:46am by George2

Chemistry
Predict whether the equivalence point of each of the following titrations is below, above, or at pH 7: Pyridine titrated with nitric acid
Tuesday, April 13, 2010 at 9:38pm by Joan

AP Chemistry
Try this. HA + NaOH ==> NaA + H2O Ka = (H^+)(A^-)/(HA) How many millimoles A- are formed when 10 mL of the base have been added? That will be 10 mL x M(whatever that is) and the concn is (10*M/V) where V is the total volume in liters. How many millimoles of the HA will ...
Tuesday, March 8, 2011 at 9:58pm by DrBob222

Chemistry
We conducted a lab with antacids in class the other day and i'm having trouble doing the calculations. Well we basically took antacid tablets dissolved them in HCl, heated it and then added phenolthalien and then titrated until we saw a pink color. At 41mL we saw the pink ...
Monday, March 15, 2010 at 8:48am by Anonymous

chem
calculate the concentration of borate ion for a titration when 6.0998g borax is dissolved in 100mL of water and titrated with 25.5mL of HCl
Tuesday, April 24, 2012 at 10:06pm by Jess

Chem Acids/Bases
WEll, you have titrated two of the protons.. .025*2Ma=.03105*.2410 solve for Molarity of the acid, Ma
Saturday, March 3, 2012 at 7:18pm by bobpursley

chemistry
A 0.446 g- sample of an unknown monoprotic acid was titrated with 0.105 M KOH. the molar mass is 120 g/mol What is the pKa value?
Monday, November 22, 2010 at 12:32am by james

chemistry
I wonder if the moles are there whether the vinegar is titrated or not? M x L = moles.
Friday, May 14, 2010 at 10:39am by DrBob222

Chemistry
Are you sure that the fact that it's titrated to 8.2-8.3 pH instead of 7.0 they are still in equal proportions? I was afraid I would have to do pKa's and -Log[conc] here
Sunday, September 20, 2009 at 2:05pm by Pavel

chemistry
what is the molarity of the acid in when a 30mL sample of HCl is titrated with 10mL of 6M NaOH?
Saturday, November 24, 2012 at 6:47pm by Boo Boo

ap chemistry
a potassium hydroxide solution is titrated with a solution of perchloric acid. what is the balanced equation?
Friday, December 31, 2010 at 7:00pm by erin

Chemistry
If you have 0.100 M Pyridine titrated with 0.100 M HCl, choose an appropriate indicator and explain?
Sunday, May 2, 2010 at 10:28pm by Andrew

Chemistry
Suppose you titrated a sample of distilled water with EDTA, approximately what volume of EDTA would be required?
Monday, October 1, 2012 at 9:41am by Julie

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

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
What is the pH when 25 mL of .20 M CH3COOH has been titrated with 35 mL of .10 M NaOH?
Monday, November 29, 2010 at 8:38pm by Louis

chemistry
50ml of 0.3M SO4 is titrated against KOH & end point is reached when 35.3 ml of the acid is added.find the molarity of the alkali
Monday, November 7, 2011 at 5:24am by Luc

chem
draw the approximate curve for a 25ml 0.10 M weak acid HA (K=1x10^-6) that is titrated with 0.10 M NaOH
Monday, January 28, 2013 at 9:53pm by rose

usm
A volume of 10.0 of a 0.190 solution is titrated with 0.770. Calculate the volume of required to reach the equivalence point.
Monday, October 29, 2012 at 9:42am by ren

chem
20ml sample of .200M HBr is titrated w/ .200M NaOH. what is the ph after adding 15ml (base)?
Sunday, April 13, 2008 at 3:10pm by ami

Chemistry
A student titrated 1.852 g of a mixture containing potassium hydrogen phthalate, KHP....? A student titrated 1.852 g of a mixture containing potassium hydrogen phthalate, KHP, with 0.163 M NaOH solution. She recorded an initial buret reading of 0.84 mL and a final buret ...
Wednesday, March 7, 2012 at 3:58pm by Cynthia

CHEM
IF A 50.0 ML SAMPLE OF CALCIUM HYDROXIDE IS TITRATED WITH 25.0 ML OF 0.200M PHOSPHORIC ACID, WHAT IS THE MOLARITY OF THE BASE?
Tuesday, May 7, 2013 at 1:14pm by SHANNA

chemistry
When 50.0 mL of 0.050 M formic acid, HCHO2, is titrated with 0.050 M sodium hydroxide, what is the pH at the equivalence point?
Wednesday, April 11, 2012 at 6:02am by chamy

chemistry
A 25 mL solution of .5M NaOH is titrated until neutralization into a 50mL sample of HCl. What was the concentration of HCl?
Tuesday, February 22, 2011 at 10:56pm by E

chemistry
thanks, sorry, 10ml of the unknown mixture was titrated methyl orange was used it took 7.5ml of 1M HCl (.0074Mol ?) so this means .00074Mol CH3NH2 / ml ?
Friday, August 24, 2012 at 8:05pm by jeffrey

chemistry
A 0.446g sample of an unknown monoproctic acid was titrated with 0.105 M KOH The molar mass is 120g/mol. What is the PKA value? Pls helps me again
Sunday, August 19, 2012 at 12:35am by Fai

chemistry
A 0.446g sample of an unknown monoprotic acid was titrated with 0.105M KOH the molar mass is 120g/mol. What is the PKA value Who helps me to solve it for me. Please help
Saturday, August 4, 2012 at 10:31pm by Fai

Chemistry
Calculate the concentration of a 50.0mL sample of HBr acid, which was titrated with 37.7 mL of 0.57 M NaOH base. Why is an overshot endpoint not a good titration?
Thursday, April 10, 2008 at 4:21pm by Jared

DrBob222 : need help with the problem
You may want a second opinion on this. If you had 5 millimoles of the carboxylic acid then you must have titrated the rest of the COOH group with the 7.5 millimoles NaOH which leaves 2.5 mmoles NaOH to titrate the other acid group whatever that may be. You must have 10 mmoles ...
Tuesday, September 11, 2012 at 12:55am by DrBob222

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