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July 24, 2014

Search: titrated

Number of results: 683

chemistry
if 50.0 mLs of HCl of unknown concentration is titrated to neutrality with 90.0 mL of .650 M NaOH. calculate the molarity of the HCl
November 14, 2011 by susan

chemistry
ph at equivalence point when 25 ml of a 0.175M solution of acetic acid is titrated with 0.10M of NaOH at its end point
March 19, 2012 by Sharnam

Chemistry
What is the molarity of a sodium hydroxide solution if 38 mL of the solution is titrated to the end point with 14 mL of 0.75M sulfuric acid?
May 1, 2012 by Emily

Chemistry
What is the molarity of a sodium hydroxide solution if 38 mL of the solution is titrated to the end point with 14 mL of 0.75M sulfuric acid?
May 1, 2012 by Emily

chemistry
A 20.0 mL sample of 0.687 M HBr is titrated with a 0.216 M NaOH solution. The pH after the addition of 10.0 mL of NaOH is __________.
July 24, 2012 by katie

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

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.
October 29, 2012 by ren

Chemistry
a 0.451 L solution of 1.71 ascorbic acid (ka1=7.9E-5, ka2=1.6E-12) is titrated with 1.35 M NaOH. What is pH when 0.9540 L of NaOH is added?
December 11, 2012 by Chris

Physical chemistry 2
50 ml of 0.02M acetic acid is titrated with 0.1M NaOH.Calculate the pH of the solution when 10ml of NaOH is added
March 12, 2013 by Anonymous

chemistry
what is a titration of 25 ml of 0.15 M HCLO2 is performed with 0.15 M NaOH. What is the pH of the solution after 25 ml of naOH have been titrated? Ka = 0.011
August 12, 2013 by auriane

Chem
A 75.0 mL volume of 0.200 M NH3 (Kb=1.8x10^-5) is titrated with 0.500 M HNO3. Calculate the pH after the addition of 28.0 mL of HNO3.
April 2, 2014 by Billy Bob Reynolds

Chemistry
A 20.0-mL sample of 0.20M sodium acetate is titrated with 0.11M HCl(aq). What is the pH after the addition of 50.0-mL HCl(aq)? (Kb of CH3CO2 = 5.6x10^-10)
March 26, 2010 by Sean

chemistry
25.0g of 5.0% (by mass) acetic acid solution are titrated with 0.300 M NaOH. What volume of NaOH will be needed to neutralize this sample?
May 28, 2010 by Cynthia

Chemistry
A solution consisting of 25.00 g Nh4Cl in 178 ml of water is titrated with 0.114M KOH. How many mL of KOH are required to reach the equivalence pt?
March 24, 2011 by Ashley

Chemistry
A 100.0 ml sample of .50 M HCl (aq) is titrated with a .10 M NaOH. What volume of the NaOH solution is required to reach the endpoint of the titration?
March 13, 2012 by Arianna

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
August 19, 2012 by Fai

Inorganic chemistry
A 50 ml sample fo 0.240M NH3(aq) is titrated with aqueous hydrochloric acid. What is the pH after the addition fo 15.0 ml of 0.0600M HCl(aq)? (kb of NH3 = 1.8 x 10^5)
April 11, 2009 by Steve

chem class
A 25.00-mL sample of 0.723 M HClO4 is titrated with a 0.273 M KOH solution. The H3O+ concentration after the addition of 10.0 mL of KOH is ???? M.
November 23, 2010 by richard

Chemistry
A 25 mL sample of wine is found to have a concentration of acetic acid of 0.23 M. If this was titrated with a 0.16 M NaOH solution how many mL's of NaOH would be required?
November 27, 2010 by Susan

Chemistry
25.0 ml of a 0.100 M solution of the weak acid, CH3OOH is titrated with a 0.10 M solution of the strong base, NaOH. Calculate the pH of the equivalence point.
February 26, 2012 by ASood

Chemistry
what is important about oxygen being formed during a titration?? (formed in container after it has been titrated not in the burette)
October 29, 2013 by Amber

chem
1. 50.00 mL of an unknown monoprotic acid is titrated with 0.132 NaOH. It takes 25.25 mL of base to reach the equivalence point. Calculate the concentration of the acid.
July 25, 2010 by Anonymous

Chemistry
How many mL of 0.139 M KOH are needed to reach the equivalence point when 1.8 g of potassium hydrogen phthalate, KHP is titrated to a phenolphthalein end-point.
October 9, 2011 by Anonymous

Chemistry
How many mL of 0.139 M KOH are needed to reach the equivalence point when 1.8 g of potassium hydrogen phthalate, KHP is titrated to a phenolphthalein end-point.
October 9, 2011 by Anonymous

chemistry
a 30.0ml sample of diprotic acid is titrated with .260M KOH. if 68.5ml is required to reach the equivalence point, what is the concentration of the acid?
October 12, 2011 by john

chemistry
25mL of tartaric acid solution is titrated against 31mL of NH4OH. What is the normality of the NH4OH? Please explain how to work this problem.
October 5, 2012 by Stephen

Chemistry
A 100.0 mL aliquot of 0.100 M weak base B (pKb=5.00) was titrated with 1.00 M HClO4. Find the pH at the following volumes of acid added Va= 0, 1, 5, 9, 9.9, 10, 10.1, and 12mL
November 14, 2012 by Missy

Balthazar
A 30 ml sample of of 0.150 m hydrazoic acid (ka = 4.50x10^-4 ) is titrated with a 0.100 m NaOH what is the ph after the ff additions of NaOH 30ml 45ml 60ml
August 1, 2013 by Omi

Chemistry
A 119.2mL sample of 0.105M methylamine (CH3NH2, Kb=3.7*10^-4) is titrated with 0.255M HNO3. Calculate the after the addition of each of the following volumes of acid. 49.1mL and 73.6mL. Please help.
February 6, 2011 by Melissa

Chem
Find and show work the final pH when 35mL of 0.200 mol/l sulfuric acid are titrated with 18mL of 0.030 mol/L sodium hydroxide?
May 26, 2010 by S.S

science
100 ml of 0.02 M acetic acid (pKa= 4.76) is titrated with 0.02 N KOH. After adding some base to the acid solution, the observed pH is 2.76. At this pH degree of protonation is
April 15, 2011 by kavin

Chemistry
A 17.6ml sample of a monoprotic acid is titrated with 0.212M NaOH. If 69.2ml of base is required to reach the equivalence point, what is the concentration of the acid?
April 19, 2013 by Chloe

chemistry
.256g unknown acid is titrated with .12M NaOH. It requires 34.8ml of base to reach the equivalence point. What is the molar mass of the acid?
May 7, 2014 by harley

Chemistry
A 50.0 mL sample of 0.10 M pyridine, C5H5N, is titrated with 0.2 M HBr. Calculate the pH to one decimal place when the following volumes of titrant have been added. 0.00 mL a) 0ml b)17ml c)25ml d)40ml
March 7, 2013 by Katie

Chemistry
Can someone please explain me how to do this problem? A 25mL solution of 0.5 M NaOH is titrated until neutralization into a 50mL sample of HCl. What was the concentration of the HCl?
February 24, 2011 by Abigail

chemistry
What chemical reaction is responsible for the endpoint observed when the NH3/NH4Cl buffer solution is titrated with HCl? Write a blanced ionic equation for the reaction.
March 27, 2011 by redgy

chemistry
A 40.0 mL sample of 0.150 M Ba(OH)2 is titrated with 0.400 M HNO3. Calculate the pH after the addtion of the following volumes of acid, and plot the pH versus millimeters of HNO3 added. a. 0.00 mL b. 10.2 mL c. 19.9 mL d. 30.0 mL e. 39.8 mL
June 27, 2011 by Cindy

chemistry
You have 20 mL of a 0.1 M aquesous solution of the weak base (CH3)3N (Kb = 7.4x10^-5). This solution will be titrated with 0.1 M HCl. how many mL of acid must be added to reach the equivalence point?
February 8, 2012 by laura

chemistry
A 20.0 mL sample of 0.687 M HBr is titrated with a 0.216 M NaOH solution. The pH after the addition of 10.0 mL of NaOH is __________. A. 0.413 B. 0.386 C. 0.163 D. 0.579 E. 0.237
July 24, 2012 by katie

Chemistry
A 20.0mL 0.3M HCl solution is titrated with 0.4M NaOH. What is the exact pH of the solution before titration? And what is the pH at the equivalence point?(are there any straightforward formulas to use on this kind of problem?)
March 18, 2013 by Sue

Chemistry
A 20.0mL 0.3M HCl solution is titrated with 0.4M NaOH. What is the exact pH of the solution before titration? And what is the pH at the equivalence point?(are there any straightforward formulas to use on this kind of problem?)
March 18, 2013 by Sue

chemistry
calculate the pH of the solution when 25.0ml of 0.0920M HCL is titrated with 0.15ml, 23.0ml, 30.0ml of 0.10M NaOH
January 23, 2013 by nathalie

chemistry
predict the pH of the solution obtained when a 1.0 M magnesium hydroxide solution is titrated with an equal amount of a 1.0 M solution of sodium chloride.
March 29, 2010 by Ash

chemistry
When a monoprotic weak acid is titrated with a strong base, the titration curve contains these many inflection points: a.zero b.one c.two d.three Can you also explain why you choose your answer to this question...thanks
March 25, 2010 by josh

AP Chem
1.513g of monoprotic acid (HX) is dissolved in water, and the volume is 250.0 ml after the dissolving. The solution was then titrated 38.12g of .100 M NaOH to reach the end point of the titration. What is the molecular weight of HX?
April 23, 2012 by Anna

Science
A 10 mL sample of tartaric acid (a diprotic acid) is titrated with 20 mL of 1.0 M NaOH. What is the molarity of the acid?
December 29, 2011 by Fahmi

ap chemistry
A titration. 12.46 mL of KMnO4 are titrated with 25 mL of H2C2O4. The half reaction is 2H2O+H2C2O4 ARROW 2H2CO3+2H+2e-. How do I get the molarity of H2C2O4? PLEASE HELP
October 11, 2010 by brian

ap chemistry
A titration. 12.46 mL of KMnO4 are titrated with 25 mL of H2C2O4. The half reaction is 2H2O+H2C2O4 ARROW 2H2CO3+2H+2e-. How do I get the molarity of H2C2O4? PLEASE HELP
October 11, 2010 by brian

Chemistry
"Find the pH of the solution obtained when 32 mL of 0.087 M ethylamine is titrated to the equivalence point with 0.15 M HCl? Do I need to do a rice table for this problem? I'm having difficulty starting this problem... Thanks!
May 21, 2007 by Rachel

Chemistry
A 30.00ml sample of 0.1234 M hypobromous acid (HBrO) is titrated with a 0.2555 M KOH solution. The Ka for HBrO is 2.5*10^-9 Calculate the pH of teh titration mixture at the equivalence point.
April 17, 2010 by Anonymous

college chem
A 0.1276 g sample of a monoprotic acid (molar mass = 1.10 x 10^2) was dissolved in 25.0 ml of water and titrated with 0.0633 M NaOH. After 10.0 ml of base has been added, the pH=5.47. What is the Ka for the acid?
March 28, 2011 by Angelina

Chemistry
A 23.0mL sample of a diprotic acid is titrated with 0.260M KOH. If 55.5mL of base is required to reach the second equivalence point, what is the concentration of the acid? I'm not sure how to do this.
February 6, 2011 by Melissa

Chemistry
I was just wondering how I would determine the pKb of a weak base that was titrated with a strong acid on a titration curve at the EQUIVALENCE POINT. And from this, how would I find the pH? PLEASE HELP!!
March 28, 2013 by TC

water chemistry
35.0 mL sample of 0.150 M acetic acid (HC2H3O2) (Ka = 1.8 x 10-5) is titrated with 0.150 M NaOH solution. Calculate the pH after 17.5 mL volumes of base have been added
April 12, 2014 by matsobane frans

water chemistry
35.0mL sample of 0.150M acetic acid9HC2H3O2)(Ka=1.8*10-5) is titrated with 0.150M NaOH solution. calculate the pH AFTER 17.5 Ml volumes of base have been added.
April 22, 2014 by mbuyelo

chemistry
what is the molarity of a sodium hydroxide solution if 26.0mL of the solution os titrated to the end point with 57.5mL of a 0.500M hydrochloric acid solution
March 8, 2013 by casey

analytical chemistry
When a monoprotic weak acid is titrated with a strong base, the titration curve contains these many inflection points: a.zero b.one c.two d.three Can you also explain why you choose your answer to this question...thanks
March 24, 2010 by josh

Chemistry
When all the following solutes act as acids, the one with the weakest conjugate base is a. H2SO3. b. H2CO3. c. HClO4. d. HClO. e. HF. 4. (Points: 1) A sample of ammonia (Kb = 1.8 * 10^-5) is titrated with 0.1 M H2SO4. At the equivalence point, the pH is approximately a. 1. b. ...
May 13, 2010 by Iby

chemistry
A 0.2481 g sample of marble was dissolved in 100 mL, and a 10.00 mL aliquot of the solution was titrated to an end point with 23.56 mL of 0.01052 M EDTA solution. What is the molecular weight? I know how to start this problem. Any help is appreciated!
October 1, 2009 by Anonymous

Chemistry
A 25.0mL sample of a 0.100M solution of acetic acid is titrated with a 0.125M solution of NaOH. Calculate the pH of the titration mixture after 10.0, 20.0, and 30.0 mL of base have been added.
November 8, 2010 by Amanda

chemistry
need math on 3. From the balanced Equation (6) and the results from step # 2 calculate the number of moles of acid titrated. (6) is CH3 COOH (aq) NaOH (aq) → Na+(aq) + CH3COO- (aq) + H2O results from #2 is 7.2*10^-3 L
February 9, 2012 by Everett

Chemistry
A solution of K2CrO4 was titrated with AgNO3, using a silver indicator electrode (E=0.799V) and a S.C.E. electrode (E=0.241V). The product, Ag2CrO4, has a Ksp = 1.1x10^-12. What is the potential at the equivalence point?
May 28, 2012 by Jeanie

chemistry
A volume of 40.0 of aqueous potassium hydroxide was titrated against a standard solution of sulfuric acid h2so4. What was the molarity of the solution if 20.02 of 1.50M h2s04 was needed? Who helps me to solve it for me.
July 31, 2012 by Fai

chem
Assume that 35.0 mL of a 0.13 M solution of a weak base B that accepts one proton is titrated with a 0.13 M solution of the monoprotic strong acid HX. (a) How many moles of HX have been added at the equivalence point?
March 24, 2013 by hannah

Chemistry
100 mL of 1.0 M formic acid (HCOOH) is titrated with 1.0 M sodium hydroxide (NaOh). The Approximate pKa is 4 At the pKa, what fraction of the carboxyl group will have been converted to COO-?
September 27, 2013 by Aria

chem help w/ Lab
Weight of the mustard package Sample: 3.02 (g) Weight of the mustard package Solution: 33.3 (g) Trial #1 Trial #2 Trial #3 Weight of Mustard Package Solution Delivered (g) : 1.09 .948 .909 Weight of NaOH Solution Delivered (g) : .354 .304 .269 Concentration of NaOH : 7.48e-3 (...
October 17, 2012 by Den

Chemisty
In titrations of acids and bases, what is the difference between the end point of the titration, and the equivalance point? Also, what is chemically occuring during the buffer zone? Thanks! Good question and one that students sometimes have trouble with. The equivalence point ...
May 15, 2007 by Jessie

science
25 ml sample of 0.150 m solution of aqueous trimethylamine is titrated with 0.100 M soultion of hcl. calculate the pH of the solution after 10.0ml,20 ml and 30.0 ml of acid have been added; pkb of (CH3)3 N =4.19?
April 19, 2010 by Jake

Chem - Titration
A 100.0-mL aliquot of 0.100 M diprotic acid H2A (pK1 = 4.00, pK2 = 8.00) was titrated with 1.00 m NaOH. Find the pH at the following volumes of base added and make a graph of pH versus Vb: Vb = 0, 1, 5, 9, 10, 11, 15, 19, 20, and 22 mL
January 23, 2012 by Meg

Titrations
How do I calcualte and what would my titration curve look like for a 25mL 0.1M H3PO4 solution titrated with 0.1M NaOh. The problem involves Ka and pKa values which i have, not sure how to use this information and make a graph out of it?
March 30, 2010 by Jerry

chemistry
Can you help me with the following: Calculate hte pH that results when 25 mL of .1M HCL is titrated with .1M NaOH solution run in from a buret at each of the stages of volume of .1 M NaOH add in 5.0 mL incrememnts beginning with 0 mL of NaOH
April 30, 2010 by Cathy

chemistry
You have 20.00 mL of a 0.1M aqueous solution of the weak base (CH3)3N (Kb = 7.4x10^-5). This solution will be titrated with 0.100 M HCl. How do you find the pH of this solution before any acid has been added.
February 9, 2012 by laura

chem 2
I just need help setting up this equation. NH3 is titrated with HCL. Does this mean the reaction is this? NH3 + HCL --> NH4 + CL- ??
July 6, 2009 by Anonymous

chemistry
When a 0.5725 g sample of Lysol was titrated with 0.100 M NaOH, and endpoint was obtained at 15.00 mL. What is the percent of HCL in the lysol sample?
June 21, 2010 by Alisha

Chemistry
A 100.0 mL sample of 0.20M HF is titrated with 0.10M KOH. Determine the pH of the solution after the addition of 100.0 mL of KOH. The Ka of HF is 3.5 x 10^-4
April 7, 2011 by Alex

chemistry
When a 0.5725 g sample of Lysol was titrated with 0.100 M NaOH, an endpoint was obtained at 15.00 mL. What is the percent of HCl in the Lysol sample?
March 22, 2012 by hank

chemistry
A 23.4 mL sample of 0.300 M trimethylamine, (CH3)3N, is titrated with 0.399 M perchloric acid. After adding 6.67 mL of perchloric acid, the pH is
April 1, 2013 by Sean

Chemistry
A 50.0 mL sample of 0.23 M propanoic acid, CH3CH2COOH, a weak monoprotic acid, is titrated with 0.14 M KOH. Ka of CH3CH2COOH = 1.4 multiplied by 10-5. What is the pH at equivalence point?
April 3, 2011 by George

Chemistry
A 30.00-mL sample of weak acid is titrated with 0.0167 M NaOH. At the endpoint , it is found the 40.35 mL of titrant was used. What was the concentration of the weak acid ?
February 22, 2012 by Cynthia

chemistry
31.0mL sample of LiOH, concentration unknown, is titrated with .52 M HCl. It takes 42.9 ml of HCl to reach the endpoint. What is the concentration of the base?
April 26, 2012 by kendra

College Chemistry
Calculate the pH at the equivalence point if 25.00 mL of 0.010M barbituric acid (HC4H3N2O3) is titrated with 0.020M NaOH. (Ka barbituric acid = 1.0 x 10^-5)
July 9, 2013 by Mary

chemistry
0.25 g of acid is titrated with .108 M NaOH. if it takes 27.22 mL of NaOH to reach the endpoint, what is the equivalent weight of the acid?
February 7, 2010 by sean

Chemistry
A volume of 25.0 ml of 0.100 M CH3C02H is titrated with 0.100 M NaOH. What is pH after the addition of 12.5 ml of NaOH? (Ka for CH3CO2H = 1.8x10-5)
October 18, 2010 by Helen

Chemistry
A 30.0-ml sample of 0.165 M propanoic acid is titrated with 0.300 M KOH. What is the pH at 5 ml of added base, at 10 ml of added base?
March 19, 2013 by Annie

Chemistry
A 50.0 mL sample of 0.51 M benzoic acid, C6H5COOH, a weak monoprotic acid, is titrated with 0.40 M NaOH. Calculate the pH at the equivalence point. Ka of C6H5COOH = 6.5 10-5. what am i supposed to do with this?
March 8, 2009 by John

chemistry
10.0 mL of 0.15M of sulfuric acid is titrated with 0.05M of sodium hydroxide. how many mL of sodium hydroxide solution are required to reach the equivalence point?
November 17, 2010 by tim

chemistry
10.0 mL of 0.15M of sulfuric acid is titrated with 0.05M of sodium hydroxide. how many mL of sodium hydroxide solution are required to reach the equivalence point?
November 17, 2010 by tim

chem
help, i'd like to know how to do this titration question: for example: a 1g sample of naoh contaminated with na2co3 is titrated with 0.500MHCl, and it is found that 46.5mL of HCl are required for neutralization. Find the percentage by mass Na2Co3. thank you in advance
April 20, 2008 by Alex

Chemistry
Okay, so here's the question: A 60.0 mL sample of 0.100M CH3COOH is titrated with 0.200M? What is the pH at each of the following points... After 30.0 mL of NaOH: This part...I'm getting confused on. I keep getting a number close to 13 and my friend is insisting that the pH is...
October 19, 2011 by Anonymous

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 ...
March 4, 2012 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 ...
March 4, 2012 by Anonymous

chemistry
Bill prepared 5.00-mL of borax solution at 59.2degrees C. He diluted the solution in an Erlenmeyer flask and titrated it to an endpoint with 27.05 mL of 0.500 M HCl. What is the saturation concentration of borate ions? I don't know what to do here. Does it involve a Ksp? Thanks
April 9, 2012 by jason

chemistry
A solution of 25mL of 0.5M c2h5nh2 is titrated with hydrochloric acid solution. During titration 5mL of .5M hcl is added dropwise. As volumes are additive. Calculate the pH of the resulting solution
April 7, 2014 by Jesus

Chemistry HELP
40.0 mL of 0.1880 M formic acid is titrated with 30.0 mL of 0.2010 M NaOH. Pka of formic acid is 3.8. What is the pH of the titration?
December 9, 2010 by Kaylee

chemistry
25 milliliters of tartaric acid solution is titrated against 31 milliliters of NH4OH. What is the normality of the NH4OH?
October 3, 2012 by Stephen

Inorganic chemistry
A 50ml sample of vinegar is titrated with 0.774M NaOH(aq). If the titration requires 41.6ml of NaOH(aq), what is the concentration of acetic acid in the vinegar?
April 11, 2009 by Steve

college chemistry
10.0 mL of 0.15M of sulfuric acid is titrated with 0.05M of sodium hydroxide. how many mL of sodium hydroxide solution are required to reach the equivalence point?
November 17, 2010 by tim

college chemistry
10.0 mL of 0.15M of sulfuric acid is titrated with 0.05M of sodium hydroxide. how many mL of sodium hydroxide solution are required to reach the equivalence point?
November 17, 2010 by tim

College Chemistry
A 20.0 Ml sample of sulfuric acid is titrated with 25.0 ML of 1.0 M NaOH solution. What is the molarity of the sulfuric acid? H2SO4+ 2NaOH yields Na2SO4 + H2O
December 6, 2010 by Sa ndra

Chemistry
A sample of 30.0 mL of sulfuric acid solution was titrated with 0.720 M KOH. It was found that 46.9 mL of the base was needed to neutralize the acid. What is [H2SO4]? would you do (30.0)(0.720) / 46.9 ?
October 12, 2011 by Hannah

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