Consider a buffer solution contains 0.20 M NaF and 0.30 M HE:-(K, (HF) = 5.0 x 104What is the pH of this solution?Choose..Calculate the pH after 0.025 mol of NAOH is added to the bufferChoose...Calculate the pH after 0.02 mol of HCI is added to the bufferChoose...

According to Handerson's equation pH = pKa + logsaltacid=-log[5×10-4]+log0.200.30=-log5-log10-4+log…

Consider a buffer solution contains 0.20 M NaF and 0.30 M HF:- (Ka (HF) = 5.0 x 104 What is the pH of this solution? Calculate the pH after 0.025 mol of NaOH is added to the buffer Calculate the pH after 0.02 mol of HCI is added to the buffer

Consider a buffer solution contains 0.20 M NaF and 0.30 M HF:- (Ka (HF) = 5.0 x 104 What is the pH of this solution? Calculate the pH after 0.025 mol of NaOH is added to the buffer Calculate the pH after 0.02 mol of HCI is added to the buffer

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter7: Neutralization Titrations And Graphical Representations

Section: Chapter Questions

Problem 1P

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Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

Consider a buffer solution contains 0.20 M NaF and 0.30 M HE:-
(K, (HF) = 5.0 x 104
What is the pH of this solution?
Choose..
Calculate the pH after 0.025 mol of NAOH is added to the buffer
Choose...
Calculate the pH after 0.02 mol of HCI is added to the buffer
Choose...

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Consider the titration of HF (K a=6.7104) with NaOH. What is the pH when a third of the acid has been neutralized?
A buffer solution is prepared by adding 5.50 g of ammonium chloride and 0.0188 mol of ammonia to enough water to make 155 mL of solution. (a) What is the pH of the buffer? (b) If enough water is added to double the volume, what is the pH of the solution?
Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations concerning weak acidstrong base titrations, the general two-slep procedure is to solve a stoichiometry problem first, then to solve an equilibrium problem to determine the pH. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong base (NaOH, for example) reacts to completion with the weak acid, HA. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak acid-strong base titration? Does the pH at the halfway point to equivalence have to be less than 7.0? What does the pH at the halfway point equal? Compare and contrast the titration curves for a strong acidstrong base titration and a weak acidstrong base titration.
A buffer solution is prepared by adding 5.50 g of ammonium chloride and 0.0188 mol of ammonia to enough water to make 155 mL of solution. (a) What is the pH of the buffer? (b) If enough water is added to double the volume, what is the pH of the solution?
Marble is almost pure CaCO3. Acid rain has a devastating effect on marble statuary left outdoors. Assume that the reaction which occurs is CoCO3(s)+ H+(aq)Ca2+(aq)+HCO3(aq) Neglecting all other competing equilibria and using Tables 15.1 and 13.2, calculate (a) K for the reaction. (b) the molar solubility of CaCO3 in pure water. (c) the molar solubility of CaCO3 in acid rainwater with a pH of 4.00.
What mass of NH4Cl must be added to 0.750 L of a 0.100-M solution of NH3 to give a buffer solution with a pH of 9.26? (Him: Assume a negligible change in volume as the solid is added.)
Consider the buffer system composed of benzoic acid, HC, H,O,, and its conjugate base benzoate, C,H,0;. HC,H,0, + H,0 = H,0* +C,H,0, Using Le Châtelier's principle, predict how the concentration of each substance changes by the addition of H,O*. Does the concentration of HC, H,0, increase or decrease when H,0* is added? O increase decrease Does the concentration of C, H,0, increase or decrease when H,O* is added? O decrease O increase Does the concentration of H,O* change significantly when H,O* is added? O no Does the concentration of H,O* change significantly when H,Ot is added? по yes Does the pH change significantly when H,O is added? no O yes Using Le Châtclier's principle, predict how the concentration of cach substance changes by the addition of OH. Does the concentration of HC,H,O, increase or decrease when OH is added? increase O decrease Does the concentration of C,H,O, increase or decrease when OH" is added? O decrease
A buffer system is prepared by combining 0.406 moles of ammonium chloride (NH4CI) and 0.525 moles of ammonia (NH3). What will the solution pH be if 0.221 moles of the nitric acid (HNO3) is added to the solution. Nitric acid is a strong acid. The K, of ammonia is 1.8 x 10-5. (Two decimal places) Type your answer... I S
An aqueous solution contains 0.32 M potassium fluoride.One liter of this solution could be converted into a buffer by the addition of:(Assume that the volume remains constant as each substance is added. More than one answer maybe required.) a) 0.32 mol HNO3 b) 0.15 mol HNO3 c) 0.31 mol HF d) 0.31 mol KI e) 0.15 mol KOH
Consider a buffer solution contains 0.20 M NaF and 0.30M HF:- (K (HF) = 5.0 x 10-4 What is the pH of this solution? Choose... Calculate the pH after 0.025 mol of NaOH is added to the buffer Choose... Calculate the pH after 0.02 mol of HCl is added to the buffer Choose... Which of the following is NOT an acid-conjugate base pair? O NaOH/ Naz0
18) What is the pH of a 100ml solution formed by adding 0.1mole NaOH to a buffer solution that contains 0.25 mole HF and 0.15 mole NaF? (K, = 6.8 x 10* for HF)
Consider a solution that contains 0.50 moles of HF and 0.50 moles of NaF in 1.0 L of water. If 0.15 mol of HCI is added to this buffer solution, the pH of the solution will get slightly The pH does not change more drastically because the HNO3 reacts with the present in the buffer system.

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