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May 6, 2016

# Search: titrated

Number of results: 835

Chemistry
If you have 0.100 M Pyridine titrated with 0.100 M HCl, choose an appropriate indicator and explain?
May 2, 2010 by Andrew

chemistry
A 40 mL sample of 0.25 M NaCHOO is titrated with 0.2 M HCl. What is the pH of the solution after 140 mL of HCl has been added?
March 2, 2011 by Eddy

CHEMISTRRY
What is the molarity of an HCl solution if 49.0 mL is completely titrated by 68.4 mL of an NaOh solution whose concentration is 0.333 M?
June 8, 2010 by Mel

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?
April 11, 2012 by chamy

Chemistry
If 25.00 ml of H2SO4 solution is titrated to an end point with 32.16 ml of 0.1986 M NaOH, what is the molarity(M) of the H2SO4 acid?
December 14, 2014 by James

chemistry
a 10.0 ml sample of a hcl solution is titrated with 32.6 ml of a 0.155 m naoh solution. what is the equation for the neutralization reaction?
November 22, 2015 by lakeisha

Chemistry
A 30.00mL sample of 0.150M KOH is titrated with 0.125M HClO4 solution. Calculate the pH after the following volumes of acid have been added: 30.0 mL, 35.0 mL, 36.0 mL, 37.0 mL, 40.0 mL
November 17, 2011 by Shana

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

chemistry
A 75.0-\rm mL volume of 0.200 M \rm NH_3 (K_{\rm b}=1.8\times 10^{-5}) is titrated with 0.500 M \rm HNO_3. Calculate the \rm pH after the addition of 13.0 mL of \rm HNO_3.
November 28, 2010 by sam

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

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 20, 2011 by Mike

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 20, 2011 by Mike

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 .75M sulfuric acid?
May 18, 2011 by Christian

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
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

chem
A 25.0 mL sample of 0.723 M HClO4 is titrated with a KOH solution. The H3O+ concentration after the addition of of KOH is
December 16, 2014 by dj westfall

chemistry
35.0 mL of an aqueous solution of HNO3 of unknown concentration is titrated with a standard solution made up of 0.453 m NaOH
May 5, 2016 by diala toulany

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

Chemistry
A 20.0-mL sample of 0.300 M HBr is titrated with 0.150 M NaOH. What is the pH of the solution after 40.3 mL of NaOH have been added to the acid?
March 5, 2015 by Jason

science
Hcl is titrated against 5ml of sodium carbonate of strength 0.0133 then what should be the mean value of HCl added ?
February 18, 2016 by Anonymous

chemistry
Hcl is titrated against 5ml of sodium carbonate of strength 0.0133 then what should be the mean value of HCl added ?
February 18, 2016 by Shareen

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
Calculate the volume at which pH = pKa if 30.00mL of weak acid with a concentration of 0.0955M is titrated against a strong base with a concentration of 0.1233M.
March 11, 2015 by Caroline

chemistry
A particular weak acid (HA) with a Ka of 2.0e-5 is 75% titrated with a strong base to produce a buffer solution. What is the pH of this final solution? Show all work.
March 24, 2015 by Nicole

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

Chemistry
I need help i do not know how to do this problem at all. A 30.00 mL sample of 0.1500 M hydroazoic acid (HN3; Ka = 1.9 x 10-5) is titrated with 0.1000 M KOH. Calculate the pH after the following volumes have been added:
August 4, 2014 by Jamie

Chemistry
A single titration was performed which required 12.60 mL of 0.100 M Na2S2O3. The density of the original, undiluted unknown bleach was 1.040 g/mL. Calculate the number of moles of ClO- in the sample titrated.
March 8, 2015 by Tori

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
In an acid-base titration, 33.12ml of 0.1177 M H2C2O4 was titrated with 0.2146 M NaOH to the end point. What volume of the NaOH solution was used?
February 1, 2015 by Steph

Chemistry
a 40.0 ml sample of ca(oh)2 was titrated with 0.0704 m hcl. the volume of hcl needed to reach equivalence point was 18.2 ml. what was the concentration of ca2+ present in the original solution?4
April 22, 2015 by Dahnrae

general chemistry
a solution of sulfuric acid was titrated with sodium hydroxide. if you took 23.7 mL of .025 M NaOH to reach the endpoint with a 5.0 mL sample of the acid what was its concentration?
October 8, 2015 by Lay

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

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

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
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.

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

chemistry
Why does a titrated sample that is fuschia with phenolphthalein turn colorless when the solution is blown into? HINT: Use chemistry and properly balanced chemical equations to support your statement.
May 13, 2015 by Nicole

chem 3
80 ml of 1.0M ch3 cooh(aq), are titrated with 2.0M KOH(aq) in the rreaction Ch3cooh(s)+ KOH(aq)reacts with kch3coo(aq)+ H2O what is the volume of potassium hydroxide was used to reach the end point of titration
March 18, 2016 by youssouf

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

Chemistry
A weak acid HA (pka=6.00) was titrated with 1.00M NaOh. The acid solution had a volume of 100ml and a concentration of .100M. Find the pH at the following volumes of added base. Vb=20ml
April 25, 2016 by Layla

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

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