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September 28, 2016

Search: Find the pH during the titration of 20.00 mL of 0.2470 M benzoic acid, C6H5COOH (Ka = 6.3 10-5), with 0.2470 M NaOH solution

Number of results: 108,834

chemistry
For each of the following primary standard acids, write the titration equation and calculate the volume of 0.100 M NaOH required for the titration: (i) 300 mg benzoic acid (C6H5COOH) (ii) 200 mg oxalic acid dihydrate (C2O4H2.2H2O) Equations: (i): C6H5COOH +NaOH->NaC6H5COO +...
April 22, 2013 by alex

Chemistry
Benzoic acid (C6H5COOH)is a monoprotic weak acid with Ka=6.30*10^-5. What is the pH of a solution of benzoic acid that is 0.559M and has 2.25*10^-2M NaOH added?
May 8, 2012 by Pippi

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
A 50.0 mL sample of 0.42 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. I know I have to set up an ICE chart, but I keep getting the wrong answer
April 12, 2010 by Chem Confused

chemistry
a student dissolves 0.625 g of pure benzoic acid in distilled water and titrated the resulting solution to the equivalence point using 40.8 mL of the standardized NaOH solution from Part a, assuming that benzoic acid has only one ionizable hydrogen, answer the following: ...
November 4, 2011 by Anonymous

Chem
What is the pH of the resulting solution if 30.00 mL of 0.100M acetic acid is added to 10.00mL of 0.100 M NaOH? For acetic acid, Ka=0.000018. I know that NaOH is a strong base and acetic acid is a weak acid. What is the equation: C6H5COOH+NaOH<--> C6H5COOH Once I get ...
February 27, 2008 by Sarah

Chemistry
Given acidity constant,Ka of benzoic acid is 6.28 X 10^-5. pH of 0.15 molar solution of this acid is ? Here is my method: Benzoic acid is a weak acid,hence it dissociates very little. So: C6H5COOH---> C6H5COO- + H+ [H+] and [C6H5COO-] are yet to be calculated,so let them be...
March 23, 2012 by Meenaakshi

chemistry
A 0.25 mol/L solution of benzoic acid, KC7H5O2 and antiseptic also used as a food preservative, has a pH of 2.40. Calculate the Ka of benzoic acid at SATP My work: C6H5COOH --> C6H5COO^- + H^+ Ka = (C6H5COO-)(H+)/ C6H5COOH I know my next steps are to use pH = log(H+) to ...
April 7, 2008 by Dustin

organic chemistry
1)Why benzoic acid is soluble in NaOH? 2)Why HCl is insoluble in titration of benzoic acid and NaOH? Benzoic is soluble in a solution of NaOH because the base forms the sodium salt with the acid to form sodium benzoate. The sodium salt is soluble. The second part of your ...
February 21, 2007 by kim

Chemistry (Acid/Base)
Consider a solution made by mixing 100 mL of 2.0 M acetic acid (Ka= 1.8e-5) with 100 mL of 0.00020 M benzoic acid (Ka= 6.4e-5). How many moles of solid NaOH must be added to the solution so that half of the benzoic acid is protonated (i.e. such that [HA] = [A-] for benzoic acid)?
April 9, 2015 by Emily

chem--need help, please!!!
Ka for benzoic acid, C6H5COOH, 6.5x10^-5. Calculate the pH of solution after addition of 10.0, 20.0, 30.0, and 40.0 mL of 0.10 M NaOH to 40.0 mL of 0.10 M Benzoic acid. PLEASE CHECK MY ANSWER!!!!! My answer is: Moles acid = 0.040 L x 0.10 M = 0.0040 Moles base = 0.010 L x 0.10...
October 20, 2010 by Andy

Chemistry
Calculate pH of a solution by mixing 15.0 mL of .50 M NaOH and 30.0 mL of .50 benzoic acid solution (benzoic acid is monoprotic, its dissociation constant is 6.5 x 10^ -5). I am not sure whether I am supposed to do it by acid-base titration way or to use the formula -log (Ka...
July 28, 2009 by Soojung

AP CHEMISTRY
Calculate the pH at the equivalence point in titrating 0.100 M solutions of each of the following with 0.080 M NaOH. a)hydrobromic acid (HBr) b)chlorous acid (HClO2) c)benzoic acid (C6H5COOH)
February 29, 2012 by DANNY

chemistry
11.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 of the following: 12.Before the titration. 13.After adding 24.9 mL of NaOH. 14.At the equivalence point. 15.After adding 25.1 mL of NaOH. ...
May 8, 2013 by Tina

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

chem
Calculate the pH at the equivalence point in titrating 0.100 M solutions of each of the following with 0.080 M NaOH. chlorous acid (HClO2) benzoic acid (C6H5COOH)
March 23, 2013 by hannah

Chemistry
You are asked to prepare a pH = 4.00 buffer starting from 1.50 L of 0.0200 M solution of benzoic acid (C6H5COOH) and some added sodium benzoate salt (C6H5COONa). a) Find the pH of the benzoic acid solution BEFORE adding the salt. b) Use the Henderson-Hasselbalck equation to ...
February 13, 2013 by Lacy

Chemistry
You are asked to prepare a pH = 4.00 buffer starting from 1.50 L of 0.0200 M solution of benzoic acid (C6H5COOH) and some added sodium benzoate salt (C6H5COONa). a) Find the pH of the benzoic acid solution BEFORE adding the salt. b) Use the Henderson-Hasselbalck equation to ...
February 13, 2013 by Lacy

Chemistry, acids and bases
(a) Find pH and pOH of 1.0 M solution of sodium benzoate, NaC6H5COO. (Ka of benzoic acid is 6.2x10^-5) (b) Calculate pH after 0.205 moles per liter of HCl was added (assume volume does not change (c) Calculate pH after 1.0 moles per liter of HCl was added (assume volume does ...
May 6, 2008 by Marissa

Chemistry
I there, this is my lab worksheet, I am having trouble filling it out. Please help me with it. Expt #1- Molecular Weight of Unknown Acid Unknown Acid: #3 Mass of Unknown solid acid transferred:1.0g Volume of volumetric flask: 100.00 mL Concentration of NaOH: 0.0989 M Aliqot of...
October 4, 2010 by Steve

Chemistry
A few questions I don't really get and need to see the work for A 50.0 mL sample of 0.55 M benzoic acid, C6H5COOH, a weak monoprotic acid, is titrated with 0.51 M NaOH. Calculate the pH at the equivalence point. Ka of C6H5COOH = 6.5 multiplied by 10-5. What is the pH of a ...
April 22, 2010 by Dubs

AP CHEMISTRY
Calculate the pH at the equivalence point in titrating 0.100 M solutions of each of the following with 0.080 M NaOH. A) benzoic acid (C6H5COOH) Ka= 6.3*10^-5 for it
March 1, 2012 by DAN

Chemistry
References Chapter 17: EOC Assume you dissolve 0.178 g of the weak acid benzoic acid, , in enough water to make mL of solution and then titrate the solution with 0.187 M . ( for benzoic acid = .) What was the pH of the original benzoic acid solution?
April 26, 2016 by Anonymous

chemistry
You weigh a sample of a monoprotic unknown acid and dissolve it in 50.00 mL of distilled water. Exactly half of this solution is titrated with Sodium Hydroxide to the phenolphthalein end point. The pH of the other half of the original solution is measured with a pH meter. The...
July 30, 2013 by faruk

Chemistry
What is [H+], [OH-], pH, and pOH for a 0.048mol/L solution of the weak benzoic acid, C6H5COOH?
December 9, 2013 by Vader

Chemistry
Expt #1- Molecular Weight of Unknown Acid Unknown Acid: #2 Mass of Unknown solid acid transferred:0.414g Volume of volumetric flask: 100.00 mL Concentration of NaOH: 0.0989 M Aliqot of acid titrated with NaOH: 25.00 mL Average volume of Naoh from titration: 13.9 mL Here's ...
October 10, 2010 by Rayana

biochemistry
The pH of 0.02M solution of a weak acid was measured at 7.6. What is the [OH-] in this solution? B) The Ka for benzoic acid is 6.4 x 10-5M. 150 ml of 0.1 M NaOH is added to 200 ml of 0.1 M benzoic acid, and water is added to give a final volume of 1 L. What is the pH of the ...
September 21, 2012 by Emma

Chemistry
Unknown Acid: #2 Mass of Unknown solid acid transferred:0.414g Volume of volumetric flask: 100.00 mL Concentration of NaOH: 0.0989 M Aliqot of acid titrated with NaOH: 25.00 mL Average volume of Naoh from titration: 13.9 mL Here's where I need help: No of moles NaOH used: ? ...
October 10, 2010 by Rayana

chemistry
Given 20g of benzoic acid contaminated with 0.4g of salicytic acid. 1)Determine the volume of hot water required to dissolve the mass of acid. 2)Calculate the mass of benzoic acid which participates when the solution is cooled to 20°C. Deduce. 3)Calculate the mass of salicylic...
October 21, 2015 by Jenny

Chemistrey
Problem: What is the heat capacity of the newly assembled oxygen bomb calorimeter? Experimental design: An oxygen calorimeter is assembled and several samples of the primary standard, benzoic acid are burned using a constant pressure of excess oxygen. The evidence that is ...
April 4, 2007 by Calorimeter

chemistry
You weigh a sample of a monoprotic unknown acid and dissolve it in 50.00 mL of distilled water. Exactly half of this solution is titrated with Sodium Hydroxide to the phenolphthalein end point. The pH of the other half of the original solution is measured with a pH meter. The...
July 30, 2013 by faruk

College Chemistry
You weigh a sample of a monoprotic unknown acid and dissolve it in 50.00 mL of distilled water. Exactly half of this solution is titrated with Sodium Hydroxide to the phenolphthalein end point. The pH of the other half of the original solution is measured with a pH meter. The...
April 9, 2013 by Kim

chemestry
When you lowered the pH of your combined aqueous NaOH extracts, you observed precipitation of benzoic acid. Explain what happened during this acidification and why the precipitation of benzoic acid occurred.
March 30, 2011 by Ami

Chemistry III
Assume you dissolve 0.240 g of the weak acid benzoic acid, C6H5CO2H, in enough water to make 1.16 102 mL of solution and then titrate the solution with 0.153 M NaOH. C6H5CO2H(aq) + OH -(aq) C6H5CO2-(aq) + H2O(l) (a) What was the pH of the original benzoic acid solution? (b) ...
March 27, 2012 by Kelly

chemistry
PLEASE NOTE: Titration requires several steps in order to obtain exact results. The procedures described in this lab assume that you have already done the TITRATION TUTORIAL and are familiar with the technique. 1. Prepare the NaOH solution by dissolving approximately 4g of ...
April 15, 2011 by Zach

chemistry
The enthalpy of combustion of benzoic acid,C6H5COOH, which is often used to calibrate calorimeters, is -3227kJ/mol. When 1.236g of benzoic acid was burned in a calorimeter, the tempurature increased by 2.345K. What is the specific heat of the calorimeter?
November 2, 2008 by annemarie

Chemistry, pH, Buffers
Please help!! Given this data: mass of unknown acid 1.4671g Volume of NaOH used in titration 18.47mL Concentration of the NaOH used 0.2403M pH of the original acid solution 2.16 pH of the final acid solution 3.49 Show me how do I calculate the Ka of the unknown acid and the ...
April 2, 2012 by Krina

Chemistry
Lab: Titration of NaOH (0.1 molar)to unknown solid acid. Trying to determine the equilivent weight of the unknown acid in the experiement. I am trying to figure out if I add too much base solution by accident to an unknown acid during titration would it affect the equivalent ...
September 26, 2012 by Dee

college chemistry
The enthalpy of combustion of benzoic acid,C6H5COOH, which is often used to calibrate calorimeters, is -3227kJ/mol. When 1.236g of benzoic acid was burned in a calorimeter, the tempurature increased by 2.345K. What is the specific heat of the calorimeter?
November 3, 2008 by annemarie

chemestry
the enthalpy of combustion of benzoic acid C6H5COOH, which is used to calibrate calorimeters usualmete is -3227 kJ mol-1. burning 1.453g of benzoic acid into a calorimeter, the 2,265 ° C temperature increase what is the heat capacity of the calorimeter?
April 23, 2015 by Daniela

Chemistry
calculate the concentration of sodium benzoate that must be present in a 2.0M solution of benzoic acid (C6H5COOH) to produce a pH of 4.00. THIS IS THE ONLY INFORMATION GIVEN. I CANNOT FIND Kb ANY WHERE IN MY TEXT NOR DOES IT GIVE US A VOLUME. CAN ANYONE HELP?
May 27, 2010 by Lucinda

Chemistry
For this question, I know how to answer the first three questions, but not the rest. 12ml 0.025 M of benzoic acid (Ka=6.3x10-5)is titrated with 0.050 M NaOH. How many moles of benzoic acid are there? I got 0.0003 What volume of NaOH is required?(L) I got 0.006 What is the ...
June 23, 2015 by Sara

organic chemistry
How to find the volume of hot water required to dissolve the mass of acid, if we have 20g of benzoic acid contaminated with 0.4g of salicylic acid? What is the mass of benzoic acid which participates when the solution is cooled to 20°C? Deduce. What is the mass of salicylic ...
October 21, 2015 by Anonymous

Chemistry, Buffers, pH
Hi could someone please help me in the next 5 minutes with this question: Given this data: mass of unknown acid 1.4671g Volume of NaOH used in titration 18.47mL Concentration of the NaOH used 0.2403M pH of the original acid solution 2.16 pH of the final acid solution 3.49 Show...
September 26, 2008 by janet

CHEM-102
Calculate the pH of a solution prepared by mixing 10.00mL of 0.50M NaOH and 20.00mL of 0.50M benzoic acid solution. (Benzoic acid is monoprotic; its ionization constant is 6.7x10^-5).
March 27, 2011 by Christian

chemistry help asap
Please check these thanks. 1. In a titration, 33.21 mL 0.3020M rubidium hydroxide solution is required to exactly neutralize 20.00 mL hydrofluroic acid solution. What is the molarity of the hydrofluroic acid solution? Answer: 0.502HF 2. A 35.00 mL-sample of NaOH solution is ...
February 6, 2012 by missy

chemistry
1. if 15.0mL of 4.5 M NaOH are diluted with water to a volume of 500mL, what is the molarity of the resulting solution? 2. in a acid-base titration, 33.65mL of an 0.148 M HCL solution were required to neutralize 25.00mL of a NaOH solution. What is the molarity of the NaOH ...
October 25, 2011 by djella

chemistry
A 0.25 mol/L solution of benzoic acid, KC7H5O2 and antiseptic also used as a food preservative, has a pH of 2.40. Calculate the Ka of benzoic acid at SATP How does the benzoic acid ionization go?
April 6, 2008 by Sarah

Chemistry
Enough water is added to 0.35 g of benzoic acid to make 1000 mL of solution. What is the pH? Ionization Constant for Benzoic Acid Ka = 6.5 × 10–5 Molar Mass Benzoic Acid 122. g·mol–1 (A) 1.9 (B) 2.6 (C) 3.4 (D) 4.2
April 15, 2008 by LT

chemistry
enzoic acid is a weak monoprotic acid with Ka = 6.5×10-5 M. NaOH(s) was gradually added to 1.00 L of 8.66×10-2 M benzoic acid. 1. Calculate the pH of the solution before the addition of the base. 2. Calculate the pH of the solution after the addition of 5.20×10-2 mol of NaOH(s).
March 25, 2014 by bekah

Chemistry
You have 150 ml of a solution of benzoic acid in water estimated to contain about 5 g of acid. The distribution coefficient of benzoic acid in benzene and water is approx 10. Calculate the amount of acid that would be left in the water solution after three 50 ml extractions ...
November 22, 2010 by Nat

Chemistry
You have 150 ml of a solution of benzoic acid in water estimated to contain about 5 g of acid. The distribution coefficient of benzoic acid in benzene and water is approx 10. Calculate the amount of acid that would be left in the water solution after three 50 ml extractions ...
November 22, 2010 by Nat

Chemistry
Consider the titration of 20.0mL of 0.300M acetic acid, HAc, with 0.150M NaOH solution. Ka=1.75*10^-5 HAc + NaOH ---> NaAc + H2O What is the composition of the solution at the equivalence point of the titration? Give both the formula of the compound and its concentration. ...
May 1, 2015 by Jonah

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
Calculate the pH at the stoichiometric point of a titration of 25.0 mL of 0.120 M benzoic acid with 0.0230 M NaOH
March 26, 2015 by lawerence

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
The student used the KHP in a subsequent titration experiment where he titrated 25.00 +/- 0.03 ml of the acid against an unknown solution of NaOH. The titration required 23.70 +/- 0.10 ml of the base. What is the concentration of NaOH?
August 9, 2015 by Aaeisha

chemistry
Determine the pH (to two decimal places) of a solution prepared by adding 395 mL of 0.0360 M benzoic acid (C6H5COOH) to 12.5 g of sodium benzoate (NaC6H5COO).
November 29, 2014 by fati

chemistry
Benzoic acid reacts with water to form the benzoate ion by the following reaction C6H5COOH(aq) + H2O(l) ⇀↽ C6H5COO−(aq) + H3O +(aq) The equilibrium constant for this reaction is 6.4 x 10−5 . In a 0.1 M solution of benzoic acid, what is the concentration...
February 7, 2015 by Anonymous

Chem
Please tell me if these are right! 1.How many milliliters of 0.215 M NaOH solution are needed to completely neutralize 2.50 ml of 0.825 M H2SO4 solution? I got 19.2 ml 2. A 10.0-ml sample of vinegar which is an aqueous solution of acetic acid HC2G3O2 requires 16.5 ml of 0.500M...
December 6, 2010 by Jessica

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
Calculate the pH of a buffered solution that is 0.100M in C6H5COOH (benzoic acid, Ka = 6.4 x 10-5) and 0.100M in sodium benzoate (NaC6H5COO).
May 5, 2010 by Rachel

chem
If 20.5 mL of a 5.256 M solution of benzoic acid is used in an experiment similar to experiment 4, how many grams of benzoic acid is in the starting solution? (molar mass of benzoic acid = 122.12 g/mol) Be sure to pay attention to significant figures. The answers are all in ...
February 4, 2013 by alice

chemistry
Find the pH during the titration of a 20.00mL of 0.1000 M butanoic acid, CH3CH2CH2COOH (Ka=1.54 x10^-5), with the addition of 10 mL of 0.1000 M NaOH solution??
April 9, 2012 by anonymous

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

Phenolphtalein vs Methyl Orange (check my reasonin
Why can either phenolphthalein or methyl orange be used for an HCl-NaOH titration, but only phnolphthalein is suitable for an acetic acid-NaOH titration? Sol: for a while,I misunderstood the question and suggested that Phenol. has a wider array of pH. But then both can be used...
June 12, 2006 by Kizner

chemistry
the titration of 25.0 mL of a 0.040 M aqueous solution of maleic acid C2H2(COOH)2, with aqueous 0.10 M NaOH solution. For maleic acid, Ka1 = 0.013 and Ka2 = 8.5 x 10-7 How many milliliters of the 0.10 M NaOH solution are needed to completely react all the maleic acid in 25.0 ...
June 30, 2013 by sue

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
You prepare a buffer solution by dissolving 2.00 g each of benzoic acid, C6H5COOH and sodium benzoate, NaC6H5COO in 750.0 mL of water. What is the pH of this buffer? Assume that the solution's volume is 750.0 mL.
April 24, 2016 by Dron

Chemistry
Find the pH during the titration of 20.00 mL of 0.1000 M butanoic acid, CH3CH2CH2COOH (Ka = 1.54e-5), with 0.1000 M NaOH solution after the following additions of titrant: 0 mL, 14.00 mL, 19.95 mL, 20.00 mL, 20.05 mL, 24.00 mL.
November 23, 2011 by James

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
Find the Molecular weight of unknown acid #5... Mass of acid #5 = 1.200g Volume (acid was mixed in) = 100ml (distilled water) Conectration of NaOH = 0.989 M Aliquot of acid titrated with NaOH = 25ml = 0.025 L Average volume of NaOH from titration = 9.3ml = 0.0093L Molar ratio ...
October 10, 2010 by AishaKay

chemistry, please help!
Given: 1. Mass of oxalic acid + weighing paper 2.0355g 2. Mass of weighing paper 0.5219 g 3.volume of oxalic acid solution 250 mL 5. Volume of oxalic acid used in titration trial 1: 15.o mL Trial 2: 15.0 mL 6. Volume of NaOH solution used in titration: Trial 1: 12.1 mL trial 2...
May 2, 2011 by Tina

Chemistry
1)What could have caused the impurity in the sodium hydroxide solution? 2)Why was it necessary to dilute the hydrochloric acid before carrying out the titration? This was a question from a titration practical in which we had to dilute HCL then use that along with 25cm3 of NaOH...
October 18, 2014 by Anon

Chemistry
How to solve titration problem for HC2H3O2 + NaOH= NaC2H3O2 + H2O The M of NaOH= 0.427 The volume of NaOH= 17.30mL 10.00mL of acid The second titration calculation is: The M of NaOH= 0.427 The volume of NaOH=34.60mL 20.00mL of acid
September 27, 2012 by John

chemistry
How to solve titration problem for HC2H3O2 + NaOH= NaC2H3O2 + H2O The M of NaOH= 0.427 The volume of NaOH= 17.30mL 10.00mL of acid The second titration calculation is: The M of NaOH= 0.427 The volume of NaOH=34.60mL 20.00mL of acid
September 29, 2012 by Anonymous

chemistry
I am confused on how to do the last question. Calculate molarity of HCl from the volumes of acid and base at the equivalence point and the molarity of NaOH from the titration curve. (M of Acid)x(v of acid)= (m of base)x(v of added base) M1= 0.50M of NaOH x 0.050L/0.01505L M1= ...
February 27, 2008 by Tim

General Chemistry 1412 inorganic
Find the pH of a solution that is 0.30 M benzoic acid (HBz) and 0.25 M sodium benzoate(NaBz). Ka for benzoic acid = 6.5 x 10-5
April 18, 2012 by generalchem1412

chemistry
(i) Give a brief explaination of the two bonding factors which determine the strength of an acid. (ii) Give a brief explanation of an Acid Buffer. (iii) Define an acid and base in terms of the Bronsted-Lowry theory. Give two examples of conjugate acid/base pairs which adhere ...
December 28, 2011 by cindy

Chemistry
In a acid-base titration, 22.81 mL of an NaOH solution were required to neutralize 26.18 mL of a 0.1121 M HCl solution. What is the molarity of the NaOH solution?
February 19, 2009 by Jake

Chemistry
1.) Watch the animation, and observe the titration process using a standard 0.100 M sodium hydroxide solution to titrate 50.0 mL of a 0.100 M hydrochloric acid solution. Identify which of the following statements regarding acid-base titrations are correct Drag items A-F to: ...
November 19, 2015 by LuigiR

Organic Chemistry - Extraction
You have 100 mL of a solution of benzoic acid in water; the amount of benzoic acid in the solution is estimated to be about 0.30 g. The distribution coefficient of benzoic acid in diethyl ether and water is approximately 10. Calculate the amount of acid that would be left in ...
October 3, 2010 by Camille

Chemisty
In the titration of total acid with sodium hydroxide, NaOH, it was determined that 36.03mL of 0.0980M NaOH was needed to neutralize all the acid in a 10.0mL aliquot of a powdered drink mix solution. In a second titration, it was determined that were 1.45 x 10^(-5) moles of ...
October 22, 2014 by Mandy

College Chemistry
I need help with this question!! a sample of pure KHP weighing .8097g dissolved in water and titrated with 40.25 mL of NaOH solution. The same NaOH solution was used to titrate a solution of a weak diprotic acid H2X. A sample of 0.18694g of the weak acid was first dissolved in...
April 25, 2012 by Emily

Chemistry
Titration of 25.00 mL of a monoprotic acid solution with 0.2269 M NaOH is: Initial NaOH = 3.96 mL Final NaOH = 38.84 mL (dif is 34.88mL) Based on data what is the molar concentration of acid? I did V x M = 0.03488L NaOH x 0.2269 = 0.079143 Not sure if I should have switched to...
December 7, 2012 by Terry

Chem
Hypothesis: A prediction of what you think the results of the project will be. Write your hypothesis before you begin the experiment and, if the experiment has more than one part, you will need a hypothesis for each section. Remember to create an ‘if-then’ statement. (Example...
November 25, 2012 by Jessica

Chemistry
Consider a weak acid-strong base titration in which 25.0 mL of 0.100 M acetic acid is titrated with 0.100 M NaOH. a) Calculate the pH after the addition of 3.00mL of NaOH. b) What is the pH of the solution before the addition of NaOH (pKa of acetic acid=4.75) I got pH= 3.88 ...
February 27, 2011 by Jon

chemistry
a 35.5 mL sample of an NaOH solution is needed to titrate a 2.08 g sample of pure benzoic acid (HC7H5O2)a solid. What is the molarity of the NaOH solution?
May 9, 2012 by b

CHEMISTRY
A 1.575 g sample of ethanedioic acid crystals, H2C2O4. xH20 was dissolved in water and made up to 250cm^3 . One mole of the acid reacts with two moles of NaOH. In a titration, 25.0 cm^3 of this solution of acid reacted with exactly 15.6 cm^3 of 0.160 mol/ dm^3 NaOH. Calculate ...
July 9, 2016 by Jack

Chemistry
Acid-Base Titrations a) How will the concentration of NaOH be affected if during the titration some of the solid potassium hydrogen phthalate was spilled during the transfer? Will the concentration of the standardized NaOH increase, decrease, or have no effect? b) How will the...
March 3, 2009 by Jake

chemistry
i am given equation CH3COOH + NaOH ---> NaCH3COO + H2O 25ml of acetic acid solution 0.025L 12ml of mid point of titration 1mol of NaOH find molar concentration i use a balanced equation it's a 1:1 ratio finding NaOH molarity = mols/litre = mols/L molarity= 1mol NaOH/0.012 ...
April 12, 2008 by unknown

chemistry
the following titration data were collected: a 10 mL portion of a unknown monoprotic acid solution was titrated with 1.12340 M NaOH and required 23.95 mL of the base solution for neutralization. calculate the molarity of the acid solution calculate the molarity of the acid ...
October 25, 2011 by Doss

chemistry 2
Titration of 50.0 mL of acetic acid reaches equivalence after delivery of 22.5mL of standardized NaOH 0.21 M. What is the initial concentration of acetic acid and what is the pH of the solution? What is the pH at equivalence? What is the pH adition of 20.0 mL of NaOH? What ...
April 14, 2014 by philip

Chemistry
In a silphuric acid (H2SO4)-Sodium Hydroxide (NaOH) acid-base titration, 17.3mL of 0.126M NaOH is needed to neutralize 25mL of H2SO4 of unknown concentration. What is the morality of the H2SO4 solution? H2SO4 (aq)+ NaOH (aq) = Na2SO4 (aq) + H2O (l)
July 1, 2014 by Dawn

chemistry
Benzoic acid and quinine are dissolved in a solution of dichloromethane. Besides the normal neutral forms for benzoic acid and quinine, will there be any other chemical form(s) present in the dichloromethane solution? (benzoic acid pKa = 4.2; quinine pKa = 8.5)
August 22, 2010 by Kay

Chemistry
15.00mL sample of a solution of H2SO4 of unknown concentration was titrated with 0.3200 N NaOH. The titration required 21.30mL of the base. What was the normality of the acid solution? what was the molarity of the acid solution?
October 5, 2015 by Mark

Chemistry
Benzoic acid and quinine are dissolved in a solution of dichloromethane. (benzoic acid pKa = 4.2; quinine pKa = 8.5) a) Besides the normal neutral forms for benzoic acid and quinine, will there be any other chemical form(s) present in the dichloromethane solution? a) What ...
September 5, 2013 by Jemma

Analytical chemistry
A dilute perchloric acid solution was standardized by dissolving 0.2445 g of primary standard sodium carbonate in 50 mL of the acid, boiling to eliminate CO2, and back-titrating with 4.13mL of dilute NaOH. In a seperate titration a 25mL portion of the acid required 26.88 mL of...
August 1, 2013 by Gloria

Chemistrey
Lab exercise 10C Calibrating bomb Calorimeter Before Molar specific enthalpies of reaction can be determined, a bomb calorimeter must be calibrated using primary standard of precisely known molar enthalpy. Complete the analysis of the investigation report. Problem: What is the...
April 4, 2007 by Calorimeter

chemistry
Benzoic Acid (HC6H5OO, 122.0 g/mol) has a Ka = 6.3 x 10-5. What is the pH of a solution that has 3.050 g of benzoic acid in enough water to make a 0.250 L solution?
March 31, 2012 by Anonymous

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