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May 24, 2015

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

Number of results: 52,795

Chemistry
The phosphoric acid in a 100.00 mL sample of a cola drink was titrated with 0.1476 M NaOH. The first equivalence point was detected after 13.32 mL of base added, and the second equivalence point after 28.65 mL. Calculate the concentration of H2PO4- in mol/L. (Hint: if only ...
January 29, 2010 by Jenna

Chem-E / Chemistry
Calculate the rate of heat required to bring 1.80mol/hr of HBr gas from 37.0 C to 434.0C at atmospheric pressure (Heat capacity of HBr is described by eq.) Cp (kJ/mol * C) = a + bT + cT^2 + dt^3 T is in C and HBr - a = 2.910x10^-2, b= -2.27x10^-7, c= 9.887x10^-9, and d= -4....
August 15, 2012 by Simon

chemistry
A certain acetic acid solution has pH = 2.14. Calculate the volume of 0.0900 M KOH required to reach the equivalence point in the titration of 35.0 mL of the acetic acid solution.
April 3, 2014 by Tessa

College Chemistry
Assuming that Ka is 1.85 *10-5 for acetic acid, calculate the pH at one-half the equivalence point and at the equivalence point for titration of 50mL of 0.100M acetic acid with 0.100M NaOH.
October 14, 2012 by Kenetria

chemistry
the equilibrium constant for the synthesis of HBr(g0 from hydrogen and bromine gas is 2.18*10 exponent 6 at 730 degrees celcius.if 3.75 mol of HBr(g) is put into a 15L reaction vessel,calculate the concentration of H2,Br2 and HBr at equilibrium
April 2, 2013 by tracy

Chemistry
Amino acid solution was made by taking 3.58 g of the dry amino acid and making it up to 1.00L in water. A 25.0 mL sample was taken and titrated with NaOH of concentration of 0.0493M, with the first equivalence point at 18.15 mL and the second equivalence point at 32.05 mL. ...
May 20, 2012 by k

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...
October 25, 2010 by Jessica

chemistry
A 25.00 mL sample of 0.4 M dimethylamine (CH3)2NH is titrated with 0.150 M HCl. What is the pH at the half-equivalence point? Not sure what to do here exactly, I'm bad with the titration problems. I know there are normally a couple tables (finding the number of moles at the ...
July 30, 2011 by 1/2 equivalence point

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
Glutamate (Glu) is the conjugate base form of glutamic acid (HGlu). The Ka of glutamic acid is 5.012 x 10^5. You titrate 50 mL of 0.10 M sodium glutamate solution with 0.05 M HCl solution. Calculate the pH of the solution at the equivalence point. Ive been trying to figure ...
July 28, 2012 by kellie

Chem Titration and pH
Calculate the pH at 0mL, 5mL,...40mL for a 10.0mL aliquote of 0.100M Na3AsO4 (weak base) titrated with 0.100M HCl pKa1 = 2.25 pKa2 = 6.77 pKa3 = 11.60 Thank you First you should write equations to know where we are in the titration. At the beginning, we have the hydrolysis of ...
October 7, 2006 by julie

college chemistry
In class, we discussed the titration of a 50.0 mL sample of 0.100 M HCL with a 0.100 M solution of NaOH. How would this system change if we used a 0.100 M solution of Sr(OH)2 instead of NaOH? To answer this question, complete each of the following: a) What volume of 0.100 M Sr...
April 21, 2010 by Aubree

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

Chemistry
A 16.6 mL portion of an HBr solution of unknown strength is diluted to exactly 247 mL. If 102.1 mL of this diluted solution requires 87.8 mL of 0.37 M NaOH to achieve complete neutralization, what was the strength of the original HBr solution?
May 1, 2011 by Sam

AP Chemistry
A very old and tired , grey haired AP Chem instructor wanted to determine the Ka of an unlabelled monoprotic acid in his stockroom. He dissolved an unknown amount of acid in an unknown amount of water and proceeded to titrate the sample with a solution of NaOH of unknown ...
February 24, 2013 by Sarah

Chemistry
A very old and tired , grey haired AP Chem instructor wanted to determine the Ka of an unlabelled monoprotic acid in his stockroom. He dissolved an unknown amount of acid in an unknown amount of water and proceeded to titrate the sample with a solution of NaOH of unknown ...
February 24, 2013 by Kat

Chemistry
A very old and tired , grey haired AP Chem instructor wanted to determine the Ka of an unlabelled monoprotic acid in his stockroom. He dissolved an unknown amount of acid in an unknown amount of water and proceeded to titrate the sample with a solution of NaOH of unknown ...
February 24, 2013 by Summer

Chem
What would a titration curve look like for 25 mL of 0.400 M NH3 (aq) with 0.200 M HCl (aq) -find initial pH -find 1/2 equivalence point pH and volume of HCl required to reach this point -find equivalence point pH and volume required to reach this point -find pH at some volume ...
July 18, 2011 by Sharon

chemistry
A 20.0 gram sample is a mixture of sodium phosphate ,sodium mono-hydrogen phosphate,sodium dihydrogen phosphate and sodium chloride. The sample is dissolved in 100.0 ml of deionized water and titrated with 1.5 M hydrochloric acid. The initial pH of the solution is pH= 12.9. ...
May 22, 2012 by bill

chemistry
A 20.0 gram sample is a mixture of sodium phosphate ,sodium mono-hydrogen phosphate,sodium dihydrogen phosphate and sodium chloride. The sample is dissolved in 100.0 ml of deionized water and titrated with 1.5 M hydrochloric acid. The initial pH of the solution is pH= 12.9. ...
May 22, 2012 by bill

chemistry
Draw the tritration curve for the neutralization of a 100ml sample of 1M solution of HCl with a .6M solution of Naoh point 1: 2 ml NaOH edded point 2: 40 ml NoOH ADDED POINT 3: EQUIVALENCE POINT 4: 80 ML NaOH added
April 3, 2011 by sam

Chemistry
In a experiment to determine the molecular weight and the Ka for ascorbic acid (vit. c.) a student dissolved 1.3713g of the monoprotic acid in water to make 50 mL of solution. The pH was monitored throughout the titration. The equivalence point was reached when 35.23 mL of the...
May 19, 2007 by Tri

Chemistry
While titrating 25.00mL of a weak acid, HA, with 0.1500M NaOH, you reach equivalence point after adding 27.00mL of the NaOH. The pH of the acid initially was 2.48. What is the dissociation constant of the acid?
October 27, 2008 by Sam

Chemistry
A student titrates 0.025 M KOH into 50.00 ml of a solution of unknown weak acid HA. Equivalence point is reached when 30.00 ml of the KOH has been added. After 15.00ml of the KOH has been added the pH of the mixture is 3.92. A. What is the concentration of HA ? B. What is Ka ...
March 10, 2011 by Patrick

Chemistry
A student titrates 0.025 M KOH into 50.00 ml of a solution of unknown weak acid HA. Equivalence point is reached when 30.00 ml of the KOH has been added. After 15.00ml of the KOH has been added the pH of the mixture is 3.92. A. What is the concentration of HA ? B. What is Ka ...
March 10, 2011 by Patrick

chemistry
need help figure out how to do these problem: 1)Calculate the pH of this solution: 1.55 X 10^-2 M HBr 2)Determine the pH of this solution: pOH = 8.3 thanks
November 30, 2010 by amy

please help analytical 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 8, 2013 by Lana

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!!!!
Determine the pH at the equivalence point in the titration of 41.0 mL 0.096 M formic acid with 0.108 M NaOH at 25oC. Calculate the pH of a solution that is 0.22 M pyridinium ion (C5H5NH+) at 25oC.
March 5, 2015 by Michelle

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

Chemistry
What volume of 14.1M HBr is required to make 250mL of 1.25M HBr solution by dilution with water?
February 4, 2011 by Kat

chemistry
what volume of a 0.272 M solution of HBr is needed for a reaction that requires 49.5 g of HBr? Answer in units of L.
September 12, 2011 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

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 - 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 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

Chem
I am doing a lab concerning pH... Why is it necessary to allow a mixture of 25mL of a 0.1M HCl solution with 20mL of a 0.08M NaOH solution to cool to room temperature? (I don't know if the actualy concentrations matter) Does it affect the pH? Yes, temperature affects the pH ...
March 7, 2007 by Marisol

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

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
Use the Henderson-Hasselbalch equation to calculate the pH of a solution that is 0.140M in propanoic acid and 0.120M in potassium propanoate
November 23, 2014 by Anonymous

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

CHEM EASY
Which indicator is best suited to determine the equivalence point of a titration of diethlyamine with HBr? pKb of diethylamine=3.16 A) phenolpthalein pKHIN ~9 B) bromo blue pKHIN ~4 C) alizarin yellow pKHIN~11 D) methyl violet pKHIN~ 1 E) phenol red pKHIN ~ 7.5 ?
January 29, 2011 by Sara

Chem
1. What is the molarity of a copper(II) dihydroxide [Cu(OH)2] solution if 25.25 mL of the solution is titrated to the equivalence point with 36.18 mL of 0.549 M prussic acid [H(CN)]? 2. What volume of a 0.138 M dihydroxyl base solution is needed to neutralize 28.47 mL of 0.745...
March 29, 2015 by TK

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
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
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
a 3.54 grams solid sample of an unknown monoprotic acid was dissolved in distilled water to produce a 47.0 mL solution at 25 degrees. This solution was then titrated with 0.2 M NaOH. The equivalence point was reached when 35.72 mL of 0.2 M NaOH was delivered. A. find the ...
April 1, 2015 by jk

chemistry help
a 3.54 grams solid sample of an unknown monoprotic acid was dissolved in distilled water to produce a 47.0 mL solution at 25 degrees. This solution was then titrated with 0.2 M NaOH. The equivalence point was reached when 35.72 mL of 0.2 M NaOH was delivered. A. find the ...
April 1, 2015 by jk

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
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
A volume of 100mL of a 0.330M HNO3 solution is titrated with 0.370M KOH. Calculate the volume of KOH required to reach the equivalence point.
October 23, 2014 by Ines

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
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
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

science
a solution of hcl of concentration 1.5 mole/liter is mixed with another solution of hbr of the same concentration. calculate: 1)ph of hcl solution alone 2)ph of the final mixture
December 12, 2010 by Mero

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

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
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
(a) The measured pH of a 0.200 M HBr solution at 25C is 0.806. Calculate the activity coefficient for H . (b) The measured pH of a 0.200 M HNO3 solution at the same temperature is 0.822. Calculate the activity coefficient for H in this solution.
February 20, 2014 by kdawg

Chemistry
calculate the pH and the pOH of an aqueous solution that is 0.035 M In HCI and 0.080 M in HBr?
July 23, 2011 by Josh

Chemistry
Calculate the pH and the pOH of an aqueous solution that is 0.025 M in HCl(aq) and 0.075 M in HBr(aq) at 25C.
October 6, 2012 by Alex

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
A 100.0mL solution containing aqueous HCl and HBr was titrated with 0.1290M NaOH. The volume of base required to neutralize the acid was 47.56mL. Aqueous AgNO3 was then added to precipitate the Cl- and Br- ions as AgCl and AgBr. The mass of the silver halides obtained was 0....
November 19, 2012 by Melia

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

Chemistry
If a chemist has a stock solution of HBr that is 10.0 M and would like to make 450.0 mL of 3.0 M HBr, how would he or she do it?
February 17, 2012 by Anonymous

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
18. Calculate H for the following reaction using Hess law H2 (g) + Br2 (g) 2 HBr (g) Experimental information 2 H+ H2 H -436.4 kJ 2 Br- Br2 H -192.5 kJ 2 H+ + 2 Br- 2 HBr H -144.8 kJ
March 26, 2015 by nona

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
Explain why the volume of 0.100 M NaOH required to reach the equivalence point in the titration of 25.00 mL of 0.100 M HA is the same regardless of whether HA is a strong or weak acid, yet the pH at the equivalence point is not the same
February 9, 2015 by kobe

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

Chemistry
Calculate the pOH of an aqueous solution of 146.6 ml of 0.000625 M HBr(aq) after dilution to 850 ml.
March 21, 2013 by Mary Ann

Chemistry
Calculate the pOH of an aqueous solution of 146.6 ml of 0.000625 M HBr(aq) after dilution to 850 ml.
March 21, 2013 by Mary Ann

Chemistry
Calculate the pOH of an aqueous solution of 146.6 ml of 0.000625 M HBr(aq) after dilution to 850 ml.
March 21, 2013 by Mary Ann

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

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