Does the pH of the solution increase, decrease, or stay the same when you add solid sodium hydrogen oxalate, NaHC2O4 to a dilute aqueous solution of oxalic acid, H2C2O4? Explain your answer using the equation below.
H2C2O4 (aq) + H2O (l)⇌ HC2O41– (aq) + H3O+ (aq)
2)Why a solution of sodium chloride and hydrochloric acid cannot act as a buffer? (b) Propose a conjugate acid/base pair which can function as a buffer.
3)
(a) Calculate the pH of a buffer solution containing 0.300 mole of KF and 0.400 mol of HF in 1.00 liter solution. (Ka of HF is 7.2*10–4)
(b) What will the pH of the buffer solution in question (a) be after the addition of 20.0 mL of 1.50 M NaOH.
4)In a titration experiment, 15.00 mL of 0.500 M NaOH solution neutralizes 20.00 mL of H3PO4 solution. What is the concentration of the H3PO4 solution?
5)
Consider the following data for four hypothetical acids:
acid |
HA |
HB |
HC |
HD |
pKa |
3.04 |
2.14 |
6.54 |
1.98 |
Which one is the strongest acid?
1.98 |
||
2.14 |
||
3.04 |
||
6.54 |
6)25.0 mL of 0.0200 M NH3 is titrated with a 0.0150 M HCl. What is the pH after 40.0 mL of the HCl solution is added?
7)
25.00 mL of 0.020 M HClO is titrated with a 0.015 M NaOH. What is the pH after 20.00 mL of the NaOH solution is added? (Ka of HClO is 3.0*10–8)
8)
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Does the pH of the solution increase, decrease, or stay the same when you add solid...
1 . If a buffer solution is 0.260 M in a weak acid (?a=8.3×10−5)and 0.480 M in its conjugate base, what is the pH? pH= 2. If a buffer solution is 0.200 M in a weak base (?b=5.0×10−5) and 0.530 M in its conjugate acid, what is the ph 3. Phosphoric acid is a triprotic acid (?a1=6.9×10−3, ?a2=6.2×10−8 , and ?a3=4.8×10−13 To find the pH of a buffer composed of H2PO4 - (aq) ) and HPO4 2− (aq) , which...
a)Calculate the change in pH that occurs when 0.00100 mol of gaseous HCl is added to a buffer solution that is prepared by dissolving 4.92g of sodium acetate(molar mass = 82.03gmol^-1) in 250 ml of 0.150 mol L^-1 of acetic acid solution? Assume no change in volume upon addition of either the sodium acetate or HCl. (Ka for acetic acid = 1.8*10^-5) b)Calculate the change in pH that occurs when 0.00100 mol of gaseous HCl is added to a buffer...
A 300.0 mL buffer solution is 0.220 M in acetic acid and 0.220 M in sodium acetate. What is the pH after addition of 0.0150 mol of HCl? What is the pH after addition of 0.0150 mol of NaOH?
In this assignment, you will calculate the pH of a solution during the course of a titration. The titration under study will be: 50 mL 0.5 M acetic acid (Ka = 1.8 x 10-5) is titrated with 0.25 M sodium hydroxide. a) Write a reaction for this titration b) Calculate the equivalence volume, and the pH at this point. c) Calculate the initial pH of the acetic acid solution Calculate the pH of the solution after d) 5 mL NaOH...
What is the pH of the buffer solution in question 2 (Recall the values were: 1.0 L buffer of 0.35 M hydrofluoric acid (HF, Ka = 3.5x10-4) and 0.68 M sodium fluoride (NaF)) after 0.031 moles NaOH are added?
What is the pH of the buffer solution in question 2 (Recall the values were: 1.0 L buffer of 0.35 M hydrofluoric acid (HF, Ka = 3.5x10-4) and 0.68 M sodium fluoride (NaF)) after 0.052 moles of HCl are added? The answer is NOT 2.65
1) Calculate the pH of a 0.026 M solution of NH4NO3. Kb of NH3= 1.8x10^-5. include both the dissociation and hydrolysis equations in the set up 2)calculate the pH of a 75 ml buffer solution containing 0.20 M of citric acid(C6H8O7, Ka= 3.2x10^-7) and 0.30 M sodium citrate. and what is the pH after adding 3.0 mlbof 1.5 M HCl to the buffer solution in that question? 3) what is the pH of 20.00 ml of 0.40 M nitrous acid(...
Calculate the pH during the titration of 20.00 mL of 0.1000 M CH3COOH(aq) with 0.2000 M NaOH(aq) after 2.5 mL of the base have been added. Ka of acetic acid = 1.8 x 10-5. QUESTION 9 Calculate the pH during the titration of 30.00 mL of 0.1000 M ethylamine, C2H5NH2(aq), with 0.1000 M HCl(aq) after 26 mL of the acid have been added. Kb of ethylamine = 6.5 x 10-4. QUESTION 10 Calculate the pH during the titration of 20.00...
In this problem you will predict the pH of a buffer solution and then predict the new pH after you add NaOH or HCl. Write your answers to three decimal places (X.XXX). The Ka of HC2H3O2 is 1.8×10−51.8×10−5. 1) Calculate the pH of a buffer made from mixing 11.011.0 mL of 0.080.08 M NaC2H3O2 and 9.29.2 mL of 0.080.08 M HC2H3O2. 2) Calculate the pH of the buffer when 5.25.2 mL of 0.0090.009 M NaOH is added to the buffer...
A 260.0 mL buffer solution is 0.200 M in acetic acid and 0.200 M in sodium acetate (For all answers express them using two decimal places) A) What is the initial pH of this solution B) What is the pH after addition of 0.0150 mol of HCl C) What is the pH after addition of 0.0150 mol of NaOH