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August 1, 2014

Search: calculate pH at equivalence point in titrating 0.120M solution of 0.08M HBr

Number of results: 46,700

chemistry
50 ml of a .1103M solution of formic acid is titrated with a .2511M NaOH. a) What is the pH before and NaOH is added? b) How many mL of NaOH solution must be added to reach the equivalence pt? c) what is the pH at the equivalence pt of the titration? d) If the titration is ...
April 7, 2013 by Jessica

Chemistry
How do I do this?? Calculate the pH at the equivalence point for the titration of 0.20 M aniline (C6H5NH2, Kb = 3.8 x 10-10) with 0.20 M HCl. [Hint: remember the dilution factor caused by addition of titrant to the aniline solution.]
October 15, 2009 by Jamie

Chemistry
What is the equivalence point in an acid-base titration? I'm supposed to do a virtual lab online and it tells you to find the equivalence point, but I don't know if that means when the pH is 7 or when the indicator changes colors.
March 24, 2009 by Katie

AP chem
A 0.345g sample of anhydrous BeC2O4, which contains an inert impurity, was dissolved in a sufficient water to produce 100ml of solution. A 20.0ml portion of the solution was titrated w/ KMnO4(aq). The balanced equation for the reaction that occurred is as follows: 16H^+(aq) + ...
January 4, 2007 by michelle

Chemistry
0.50 M HI with 0.10 M KOH pH at equivalence point? I had another problem like this and I tried to do it the same way b/c I thought that was the right thing to do but it seems as if its not? Can you help? HI + KOH ==> KI + H2O. At the equivalence point we will have KI (the ...
April 2, 2007 by Paul

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 - Science
In an acid-base experiment at 25.0C, a sodium hydroxide solution was standardized against KHP. The average value for the concentration of the sodium hydroxide solution was calculated to be 0.0125 M. This solution was used to titrate the phosphoric acid present in coke. The ...
March 2, 2014 by Anonymous

Physics
a lunar landing module is descending to the moon's surface at a steady velocity of 10 m/s. At a height of 120m, a small object falls from its landing gear. Taking the moon's gravitational acceleration as 1.6m/s^2, at what speed, in m/s, does the object strike the moon? ...
November 16, 2006 by Sean

College Chemistry - Science
In an acid-base experiment at 25.0C, a sodium hydroxide solution was standardized against KHP. The average value for the concentration of the sodium hydroxide solution was calculated to be 0.0125 M. This solution was used to titrate the phosphoric acid present in coke. The ...
March 2, 2014 by Anonymous

chemistry
A 1.0 M acetic acid solution (CH3COOH, pKa = 4.7) is neutralized by dissolving NaOH(s) (a strong base) in the solution. Estimate the pH at the equivalence point of the neutralization process: 4.7 7.0 9.3 Which one of the following statements best explains your prediction? 1. ...
March 31, 2014 by bekah

chemisry
A 0.1 molal solution of a weak monoprotic acid was found to depress the freezing point of water 0.1930C. Determine the Ka of the acid. You can assume 0.1 molal and 0.1 molar are equivalent. 100 ml of a 0.1M solution of the above acid is titrated with 0.1 M NaOH. After an ...
February 12, 2012 by ashley

chemistry
What is the molarity of an HCl solution if 38.5 mL of it is titrated to the equivalence point with 41.6 mL of a 1.41 M NaOH solution?
January 13, 2013 by Megan

chemistry
a. A 0.1 molal solution of a weak monoprotic acid was found to depress the freezing point of water 0.1930C. Determine the Ka of the acid. You can assume 0.1 molal and 0.1 molar are equivalent. b. 100 ml of a 0.1M solution of the above acid is titrated with 0.1 M NaOH. After an...
February 12, 2012 by billy

chemistry
how do i calculate the [OH-] and [Ca2+] using the equivalence point? Then I have to calculate the Ksp for calcium hydroxide.
November 1, 2011 by Kris

chemistry
Consider the titration of 21.0 mL sample of 0.110 M HC2H3O2 with 0.130 M NaOH. what is the initial pH? what is the volume of added base required to reach equivalance point? what is the pH at 5.00 mL of added base? pH at one half o the equivalence point? pH at the equivalence ...
July 29, 2010 by Ellen

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

college chemistry
Suppose you have a 0.200 M solution of the nitrogen-containing weak base NX. Suppose you wish to titrate 25 mL of this 0.200 M NX solution with a 0.100 M solution of the strong acid HNO3. Given that the Kb value of NX is 6.50x10-5, complete each of the following: a) What ...
April 21, 2010 by Aubree

chemistry
A volume of 100mL of a 0.800 M HNO3 solution is titrated with 0.640 M KOH. Calculate the volume of KOH required to reach the equivalence point.
August 6, 2012 by LL

chemistry
determine the solubility product of the slightly soluble salt calcium oxalate,cac2o4 by titrating 200cm^3 sample of a suturated solution of this salt with 0.00135mol dm^3 HCl solution.calculate Ksp?
August 6, 2012 by promise

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...
May 9, 2008 by Amy

chemistry
A 20.0 mL sample of an aqueous HClO3 solution is titrated with a 0.0275 M KOH solution. The equivalence point is reached with 28.5 mL of the base. The pH of the HClO3 solution, before titration, is
March 13, 2012 by Maggie

chemistry
What is the molarity of the acetic acid if 0.5ml of a vinegar solution has been titrated with the 0.101M solution of NaOH and the volume of the NaOH solution at the equivalence point is 5.0mL?
May 13, 2013 by RC

CHEMISTRY
Ethylamine, CH3CH2NH2, is an organic base with pKb = 3.367 at 298 K. In an experiment, a 40.0 mL sample of 0.105 mol L-1 CH3CH2NH2 (aq) is titrated with 0.150 mol L-1 HI(aq) solution at 298 K. (a) Write a balanced chemical equation for the neutralization reaction upon which ...
November 27, 2012 by sabrina

CHEMISTRY
Ethylamine, CH3CH2NH2, is an organic base with pKb = 3.367 at 298 K. In an experiment, a 40.0 mL sample of 0.105 mol L-1 CH3CH2NH2 (aq) is titrated with 0.150 mol L-1 HI(aq) solution at 298 K. (a) Write a balanced chemical equation for the neutralization reaction upon which ...
November 28, 2012 by sabrina: PLease someone help!

CHEMISTRY
Ethylamine, CH3CH2NH2, is an organic base with pKb = 3.367 at 298 K. In an experiment, a 40.0 mL sample of 0.105 mol L-1 CH3CH2NH2 (aq) is titrated with 0.150 mol L-1 HI(aq) solution at 298 K. (a) Write a balanced chemical equation for the neutralization reaction upon which ...
November 28, 2012 by sabrina: I am having difficulties with this!

CHEMISTRY
Ethylamine, CH3CH2NH2, is an organic base with pKb = 3.367 at 298 K. In an experiment, a 40.0 mL sample of 0.105 mol L-1 CH3CH2NH2 (aq) is titrated with 0.150 mol L-1 HI(aq) solution at 298 K. (1a) Write a balanced chemical equation for the neutralization reaction upon which ...
November 28, 2012 by sabrina: Please help

CHEMISTRY
Ethylamine, CH3CH2NH2, is an organic base with pKb = 3.367 at 298 K. In an experiment, a 40.0 mL sample of 0.105 mol L-1 CH3CH2NH2 (aq) is titrated with 0.150 mol L-1 HI(aq) solution at 298 K. (1a) Write a balanced chemical equation for the neutralization reaction upon which ...
November 28, 2012 by sabrina: Please help

chemistry
Consider a 20.0mL sample of 0.105M HC2H3O2 is titrated with 0.125M NaOH. Ka=1.8x10^-5. Determine each of the following: a) the initial pH b) the pH at 5.0mL of added base c) the pH at one-half of the equivalence point d) the pH at the equivalence point
November 15, 2010 by bobjahng2

AP Chemsitry
A solution of an unknown monoprotic weak acid was titrated with 0.100 M NaOH. The equivalence point was reached when 37.48 ML of base had been added. From a second buret, exactly 18.74 of 0.100 M HCl were added to the titration solution. The pH was then measured with a pH ...
April 1, 2012 by Keith

Chemistry
When titrating a weak base with a strong acid, what effect will washing the tip of the burette and sides of the beaker with distilled water have on the pKa and equivalence points?
March 31, 2013 by C

Chemistry
When titrating a weak base with a strong acid, what effect will washing the tip of the burette and sides of the beaker with distilled water have on the pKa and equivalence points?
March 31, 2013 by C

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 20.0mL 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
3) A student dissolves a 1.18g aspirin tablet in water and titrates the solution with a .265M NaOH. 22.05mL of NaOH are required to reach the equivalence point. Calculate the percentage of acetylsalicylic acid in the tablet.
October 25, 2010 by Juliet

Chemistry
Sodium hypochlorite, NaClO, is added as a disinfectant to the water supply. You are analyzing a sample from the supplier to verify its purity and you prepare to titrate 250.0 mL of a solution containing 1.86 g of NaClO with a 1.00 M HCl solution. What is the pH of the solution...
February 13, 2012 by Rosa

Chemistry
What is the pH for the potassium propionate solution at the equivalence point?
May 3, 2011 by Mira

chemistry
A chemistry student weighs out 0.172 grams of acrylic acid (HCH2CHCO2) into a volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.1800 moles/liter NaOH solution. Calculate the volume of NaOH solution the student will need to add ...
January 25, 2012 by Lucas

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
A chemistry student weighs out 0.123 grams of chloroacetic acid into a 250. milliliter volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.2100 moles/liter NaOH solution. Calculate the volume of NaOH solution the student will need...
January 19, 2012 by Deborah

Chemistry
chemistry student weighs out 0.123 grams of chloroacetic acid (HCH2ClCO2) into a 250. milliliter volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.1200 moles/liter NaOH solution. Calculate the volume of NaOH solution the student...
January 19, 2012 by Deborah

Chemistry
A chemistry student weighs out 0.123 grams of chloroacetic acid (HCH2ClCO2) into a 250. milliliter volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.1200 moles/liter NaOH solution. Calculate the volume of NaOH solution the ...
January 19, 2012 by Deborah

Chemistry
A chemistry student weighs out 0.123 grams of chloroacetic acid (HCH2ClCO2) into a 250. milliliter volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.1200 moles/liter NaOH solution. Calculate the volume of NaOH solution the ...
January 19, 2012 by Deborah

Chemistry titrations
25.00mL of an unknown sulfuric acid solution is titrated to the second equivalence point with 21.02mL of 0.420M potassium hydroxide solution. What is the concentration of the sulfuric acid solution?
March 27, 2013 by Jaden

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

Analytical chemistry help!
Calculate the pH of a solution made by mixing 50.00 mL of 0.100 M NaCN (Ka of HCN = 6.2 x 10-10) with a) 4.20 mL of 0.438 M HClO4 and b) 11.82 mL of 0.438 M HClO4. What is the pH at the equivalence point with 0.438 M HClO4?
November 26, 2011 by Remy

chemistry
An HNO3 solution has a pH of 3.04. What volume of 0.015 M LiOH will be required to titrate 89.0 mL of the HNO3 solution to reach the equivalence point?
January 5, 2012 by Anonymous

chemistry
A solution of NaOH with pH 13.68 requires 35.00 mL of 0.128 M HClO_4_ to reach the equivalence point. What is the volume of the NaOH solution?
March 8, 2012 by Savannah

chem
How is the number of moles of NaOH affected at the equivalence point of the solution?
October 18, 2009 by me

Chemistry
Suppose 50.0 mL of an aqueous solution containing an unknown monoprotic weak acid is titrated with 0.250 M KOH. The titration requires 31.52 mL of the potassium hydroxide solution to reach the equivalence point. What is the concentration (in molarity) of the unknown acid ...
March 5, 2012 by Chill

chemistry
A 27.00 mL sample of an unknown H3PO4 solution is titrated with a 0.110 M NaOH solution. The equivalence point is reached when 25.78 mL of NaOH solution is added. What is the concentration of the unknown H3PO4 solution? The neutralization reaction is: H3PO4(aq) + 3NaOH(aq) -&...
September 27, 2012 by Amanda

chemistry
Calculate the boiling point elevation of a solution containing 22.8 g of glucose (C6H12O6) dissolved in 672.0 g of water. Calculate the freezing point depression for the same solution.
February 28, 2010 by mandy

chemistry
Calculate the boiling point elevation of a solution containing 22.8 g of glucose (C6H12O6) dissolved in 672.0 g of water. Calculate the freezing point depression for the same solution.
February 28, 2010 by mandy

Chem
What is different about neutralization reactions that produce a neutral solution at the equivalence point and those that produce acidic or basic solution? I think it is the concentration of the reactants?
May 20, 2013 by Anonymous

chemistry
a sodium hydroxide solution was prepared according to the procedure outlined in this weeks experiment. This sodium hydroxide solution was standardized by by titration against exactly 10mL of a 0.28M hydrochloric acid solution. In three titrations, the volumes of the sodium ...
November 25, 2012 by Kacie

Chemistry
What is the pH at the equivalence point when 0.10 M HNO_3 is used to titrate a volume of solution containing 0.30 g of KOH?
November 21, 2012 by Josh G.

Chemistry
Question: A 0.400 g sample of propionic acid was dissolved in water to give 50.00 mL of solution. This solution was titrated with 0.150 M NaOH. what was the pH of the solution when the equivalence point was reached? I'm not really sure how i would go about setting this up. ...
April 15, 2009 by Eliz

Chemistry
Hello, I have a question that reads: Using the average molarity of your initial acetic acid solutions, the initial volumes, and the volume of NaOH added to reach the equivalence point, calculate the [C2H3O2-] concentration at the equivalence point. You should report 4 ...
May 9, 2010 by Jens

chemistry
A compound was found to be composed of the following amounts of elements: 20.00% wt% C, 26.64wt% O, 46.65 wt%N, and 6.71wt%H. A 6.125 grams sample of this compound dissolved in 46.205 grams of water as a solution was found to have a freezing point of -3.260C. The density of ...
April 25, 2013 by lucy

Chemistry
The following data was obtained from titrating a solution containing 25 mL of 0.0100 M MgCl2 solution, 1 mL of NH3OH buffer, and 10 drops of Calmagite with EDTA. Calculate the concentration of EDTA. Report the answer with three sig figs. Please help it only shows a graph with ...
May 13, 2013 by shannon

chemistry
For the titration of 50.00 mL of 0.1000 M ammonia with 0.1000 M HCl, calculate the pH (a) before the addition of any HCl solution, (b) after 20.00 mL of the acid has been added, (c) after half of the NH3 has been neutralized, and (d) at the equivalence point.
April 11, 2012 by chamy

Chem
if 0.24o moles of a monoprotic weak acid is titrated with NaOH, what is the PH of the solution at the 1/2 equivalence point.
March 10, 2014 by Joe

Chemistry
It says prepare a theoretical titration of 25 mL of 0.1037 M formic acid (HCOOH; pKa= 3.75) solution (diluted to 100mL volume with deionized water) by 0.0964 M solution of KOH. It asks to determine the volume of KOH solution needed to reach equivalence point. But I don't even ...
October 25, 2010 by Anonymous

Chemistry
10.00 mL of an unknown base solution is titrated with .100 M HCl solution. The pH versus the volume of NaOH added is shown below. There is a graoh where there are two dotted lines signifying a pH: the highest at pH 6.31 and the lower at pH 3.92. What is the pOH pf the solution...
March 27, 2014 by Dezzi

Chemistry
Calculate the theoretical pH at the starting point and at each equivalence point for phosphoric acid, acetic acid, and sulfuric acid. Please show the equilibrium equation, the Ka, and the pH calculation.
December 12, 2011 by Shana

Chemistry
give a formula you can use to calculate the number of moles of H+ ions used at the equivalence point.
October 26, 2011 by Emma

Chemistry
calculate the pH at 0ml at the quivalence point and at 40ml in a titration of 25 ml of .120M formic acid with .105M NaOH (kA of formic acid= 1.8x10^-4)
March 1, 2009 by Gagan

analytical chemistry
your lab possesses a stock solution of NaOH whose concentration is approx. 0.1M. you prepare a secondary solution by diluting 15.00mL of this stock solution to a total volume of 250.0 mL. you titrate a 50.00mL aliquot of the secondary solution with a hydrochloric acid solution...
February 21, 2013 by holly

Chemistry
Hello, i seem to be stuck on a problem and do'nt know why im not gettin the right answer.I have the he Ka and Kb values for each of the weak acids and bases from the chart and I keep getting zero and the second one 2.27*10^-24 is this correct?? Thank uu Solve an equilibrium ...
March 24, 2011 by Amy Wight

Chemistry
Hello, i seem to be stuck on a problem and do'nt know why im not gettin the right answer.I have the he Ka and Kb values for each of the weak acids and bases from the chart and I keep getting zero and the second one 2.27*10^-24 is this correct?? Thank uu Solve an equilibrium ...
March 24, 2011 by Amy Wight

Chemistry
Hello, i seem to be stuck on a problem and do'nt know why im not gettin the right answer.I have the he Ka and Kb values for each of the weak acids and bases from the chart and I keep getting zero and the second one 2.27*10^-24 is this correct?? Thank uu Solve an equilibrium ...
March 24, 2011 by Amy Wight

Chemistry
1. A solution is prepared such that it is 0.45 M in formic acid and 0.35 M in sodium formate. a) Where is this mixture located on a titration curve: before the buffer point, at the buffer point, or after the buffer point? b) Use the Henderson-Hasselbach to determine the pH of ...
July 15, 2014 by Arthur T

Chemistry
Calculate the boiling points of freezing points of the following solutions in water. a) boiling point of a 2.25m solution of propylene glycol (a non-electrolyte) b)freezing point of a 1.0m solution of potassium iodide c)freezing point of a 1.0m solution of nickel(II) nitrate d...
May 2, 2010 by Ralph

Chemistry 2
A titration is performed by adding 0.124 M KOH to 40 mL of 0.159 M HNO3. a) Calculate the pH before addition of any KOH. b) Calculate the pH after the addition of 10.26, 25.65 and 50.29 mL of the base.(Show your work in detail for one of the volumes.) c) Calculate the volume ...
April 2, 2013 by Antonio

Jill
State the relationship of A to B (i.e. <, >, = or can't be determined). 1. Using a 0.05 M Ag+ titrant A.VEP in titration 25-mL of 0.01 M MgCl2 B.VEP in titrating 25-mL of 0.01 M AlCl3 2. A 25.0-mL solution contains 0.015 M NaCl and 0.010 M HCl A.VEP (Mohr) B.VEP (...
February 20, 2012 by Chemistry Homework Help

Chemistry
A solution contains 15 g non-volatile non-electrolyte solute C6H14O6 dissolved in 500 g of water at 40 c. Calculate (A)Vapor pressure of the solution. (B)Boiling point of the solution. (C)Freezing point of the solution.
September 1, 2012 by Yeneta

CHEMISTRY
1. What is the vapor pressure at 25C of a solution of 1.20g of nephtalene C10H8 in 25.6g of benzone C6H6? The vapor pressure of pure benzene at 23C is 86.0mmHg the vapor pressure of naphthalene can be neglected. Calculate the vapor pressure lowering of the solution. 2. A ...
March 20, 2013 by N COMAS

Chemistry
how many milliliters of 0.0850 m naoh are required to titrate 50.0 ml of a solution that contains 1.85 g of hcl per liter to the equivalence point?
February 22, 2011 by Charles Maxey

Chemistry
1) What is the vapor pressure at 25C of a solution of 1.20g ofnephtalene C10H8 in 25.6g of benzone C6H6? The vapor pressure of pure benzene at 23C is 86.0mmHg the vapor pressure of naphthalene can be neglected. Calculate the vapor pressure lowering of the solution. 2)A ...
March 19, 2013 by N comas

Chemistry
Calculate the pH at the equivalence point for the titration of 0.130M methalamine (CH3NH2) with 0.13M Hcl. The Kb of methyl amine is 5.0x10-4.
March 18, 2013 by Joe

chem
why is it necessary to heat the oxalic acid solution before titrating it with the potassium permanganate solution
July 20, 2008 by mAddee

chemistry
Suppose that 50mL of a solution of sulfuric acid of unknown concentration was titrated with a 0.100M solution of sodium hydroxide. If it took 45.5 mL of titrant to reach the equivalence point, what was the concentration of the unknown solution of sulfuric acid???
July 7, 2013 by Coach

Chemistry 20 titration
1) oi50 . tinypic . com / ejh6vm . jpg The most suitable indicator for the titration is: A)methyl violet B)chlorophenol red C)methyl orange D)phenolphthalein 2-A base is titrated with an acid solution until the indicator changes colour. This change in the colour of the ...
October 22, 2012 by Rock

Chemistry
You are titrating 35.00 mL of a 1.20 M solution of HCOOH with a strong base. If you add 1.00 mL of a 3.60 M solution of sodium hydroxide, what is the final pH of the acid solution? The Ka for HCOOH is 1.8 X 10-4.
February 24, 2011 by Carl

Science (chemistry) help please
The following data was obtained from titrating a solution containing 25 mL of 0.0100 M MgCl2 solution, 1 mL of NH3OH buffer, and 10 drops of Calmagite with EDTA. Calculate the concentration of EDTA. Report the answer with three sig figs. I don't know what to do? I know that 0....
May 14, 2013 by andy

Chemistry
Assume you dissolve 0.235 g of the weak acid benzoic acid, C6H5CO2H, in enough water to make 4.00*10^2 mL of solution and then titrate the solution with 0.138 M NaOH. C6H5CO2H(aq) + OH-(aq) C6H5CO2-(aq) + H2O(l) Find concentration of Na+ at equivalence point.
April 21, 2013 by john

Chemistry
10. For the titration of 20.00 mL 0.1000 M lactic acid with 0.1000 M NaOH, calculate the pH: a. before any titrant is added b. 10.00 mL prior to the equivalent point c. at the equivalent point d. 10.00 mL after the equivalence point. Plot the points obtained on a graph of pH ...
June 22, 2014 by Rick

Chemistry
Can anyone answer this question please. (Determine the concentration of an aqueous NaCl solution if 31.5 mL are required to reach the equivalence point when titrated with 25.0 mL of 0.20 M AgNO3.)
September 19, 2010 by John

chemistry
a solid sample of impure Ba(OH)2 is added to 400.0 mL of 0.5000 M of aqueous HBr, a strong acid. the remaining solution was acidic. it was then titrated to equivalence point with 120.0 mL of 0.5000 M of NaOH solution. what mass of pure Ba(OH)2 was present in the sample?
February 26, 2011 by mel <3

chemistry
A 13.0 mL sample of an unknown HClO4 solution requires titration with 25.2 mL of 0.180 M to reach the equivalence point. What is the concentration of the unknown HClO4 solution? The neutralization reaction is as follows: HClO4 +NaOH ===>> H2O +NaClO4
November 2, 2010 by john

physics college
An antelope moving with constant acceleration covers the distance between two points 70.0 m apart in 7.00 s. Its speed as it passes the second point is 15.0 m/s. (a) What is its speed at the first point? (b) What is its acceleration? A car is stopped at a traffic light. It ...
October 8, 2010 by meera

chemistry
What volume in mL of 0.0985 M sodium hydroxide solution is required to reach the equivalence point in the complete titration of a 15 mL sample of 0.124 M phosphoric acid?
December 9, 2012 by What?

chemistry
What volume in mL of 0.0985 M sodium hydroxide solution is required to reach the equivalence point in the complete titration of a 15 mL sample of 0.124 M phosphoric acid?
December 10, 2012 by What?

chemistry
Calculate the pH at the equivalence point for the titration of 0.25 M CH3COOH with 0.25 -5 M NaOH. (For CH3COOH, Ka= 1.8 ⋅ 10 )
July 15, 2013 by ginger

Chemistry
Calculate the pH at the equivalence point for the titration of 0.120 M methylamine with 0.120 M HCl (kb of methyalamine is 5.0 x 10^-4)
November 13, 2011 by Mariana

Chemistry
Suppose a student titrates a 10.00-mL aliquot of saturated Ca(OH)2 solution to the equivalence point with 13.65 mL of 0.0234 M HCl. What was the initial [OH − ]? What is the experimental value of Ksp?
February 5, 2014 by Kelly

chemistry
5Fe(2+ charge) + MnO4(-1 charge) +8H(1+ charge) -> 5Fe(3+ charge) + Mn(2+ charge) + 4H2O In a titration experiment based on the equation above, 25ml of an Acidified Fe(2+ charge) solution requires 14 ml of standard .050 M MnO4(1- charge) solution to reach the equivalence ...
October 3, 2007 by corey

Chemistry
A solution of magnesium chloride, MgCl2, is prepared by dissolving 19.0g of MgCl2 in 250 mL OF water. a.) Calculate the weight percent of magnesium chloride in solution. b.)The denstiy of the above solution is 1.05 g/mL. Calculate the molarity of the magnesium chloride ...
October 24, 2012 by Josh

Chemistry
During an acid-base titration, 25 mL of NaOH 0.2 M were required to neutralize 20 mL of HCl. Calculate the pH of the solution for each: a) Before titration b) After adding 24.9 mL of NaOH c) At equivalence pt d) After adding 25. 1 mL of NaOH e) The pH of the equivalence pt ...
May 10, 2014 by al

Chemistry
A .682 g sample of an unknown weak monoprotic acid, HA, was dissolved in sufficient water to make 50mL of solution and was titrated with a .135 M NaOH solution. After the addition of 10.6mL of base, a pH of 5.65 was recorded. The equivalence point was reached after the ...
May 9, 2007 by Sara

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