Answered: How many grams of NaF ( molar mass =…

How many grams of NaF ( molar mass = 41.99 g/mol) would be needed to be added to 2.00 L of 0.100 M HF ( pKa = 3.18) to form a solution with pH = 4.00?

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 14QAP: A buffer solution is prepared by adding 5.50 g of ammonium chloride and 0.0188 mol of ammonia to...

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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.

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How many grams of NaF ( molar mass = 41.99 g/mol) would be needed to be added to 2.00 L of 0.100 M HF ( pK_a = 3.18) to form a solution with pH = 4.00?

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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?
Enough water is added to the buffer in Question 29 to make the total volume 10.0 L. Calculate (a) the pH of the buffer. (b) the pH of the buffer after the addition of 0.0500 mol of HCl to 0.600 L of diluted buffer. (c) the pH of the buffer after the addition of 0.0500 mol of NaOH to 0.600 L of diluted buffer. (d) Compare your answers to Question 29(a)-(c) with your answers to (a)-(c) in this problem. (e) Comment on the effect of dilution on the pH of a buffer and on its buffer capacity.
A chemist starts her experiments with 25.00 mL of 0.125 mol L-1 NaCN solution. The pKa of HCN = 9.20. a) What volume of 0.100 mol L-1 HCl will be required to fully react with the above salt? b) After the reaction in part (a) takes place, will the pH of the solution be acidic, basic or neutral? c) What volume of 0.100 mol L-1 HCl is needed to adjust the pH of the originally provided solution to pH = 9.00? HINT: At pH 9.00, what kind of solution is created if the pKa of HCN is 9.20
A 100.mL of 0.250 M HNO2 is added to 200.mL of 0.100 M NaNO2. What is the concentration of HNO2 and NaNO2 once two solutions are mixed? What is the pH of this solution? Write a balanced equations showing what happens when NaOH is added, and when HCl is added to solution (b). What is the CHANGE in pH when 50.0 mL of 0.15 M NaOH have been added to solution (b)? What is the CHANGE in pH when 50.0 mL of 0.15 M HCl have been added to solution (b)?
A Titration of 10.0 mL of 0.15 M NaOH is added 0.35 M HNO3. What is the volume of HNO3 to reach equivalent point? 40.0 mL of 0.350 M CH3NH2 is titrated with 0.280 M HCI until the end point is reached. What is the pH of the solution at the end point. (Kb for CH3NH2 = 5.0 X 10^-4)
3) Please don't provide handwritten solution.
A 25.0 mL sample of 0.150 M benzoic acid is titrated with a 0.150 M NaOH solution, What is the pH after 26.0 mL of base is added? The K, of benzoic acid is 6.3 · 105, O 11.47 O 2.54 O 7.00 4.18 4.22 O O O O O
The graph below shows the titration of 3.00 mL of a weak monoprotic acid (HA) solution by a 0.105 mol/L NaOH solution.Show the calculations. (a)What is the pH of the resulting solution after adding the 10.14mL NaOH solution? Given: pKw = 14.0.(b)What is the mass in grams of NaOH that must be added to 200 mL of a 0.11 mol/L acetic acid solution (pKa = 4.75) to obtain a buffer solution with a pH of 5.65?
A buffer solution is prepared from equal volumes of 0.200 M acetic acid and 0.600 M sodium acetate. Use 1.80 × 10−5 as Ka for acetic acid.(a) What is the pH of the solution?(b) Is the solution acidic or basic?(c) What is the pH of a solution that results when 3.00 mL of 0.034 M HCl is added to 0.200 L of the original buffer?
A buffer is prepared by adding 4.8 g of (NH4)2SO4 to 425 mL of 0.258 M NH3. Assuming that the volume stays constant, what is pH of the buffer solution? Consider: Kb (NH3) = 1.8×10–5, and Molar Mass of (NH4)2SO4 = 132.14 g/mol. (A) 10.04 (B) 5.22 (C) 9.44 (D) 4.93 (E) 1.75
A 100. mL sample of 0.10 M HCl is mixed with 50. mL of 0.14 M NH3. What is the resulting pH? (Kb for NH3 = 1.8 × 10–5)
Determine the pH at the point in the titration of 40.0 mL of 0.200 M HC4H,O2 with 0.100 M Sr(OH)2 after 100.0 mL of the strong base has been added. The value of Ka for HC4H;O2 is 1.5 × 10-5 1 2 NEXT > Use the table below to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of liquid water in the reaction. HC4H;O2(aq) + OH (aq) H20(1) + C4H,O2 (aq) Before (mol) |Change Imol) After | (mol) RESET 0.100 0.200 +x 0.100 + x 0.100 - x -x 0.200 + x 0.200 - x 2.00 x 103 -2.00 x 103 8.00 x 103 -8.00 х 10"3 1.00 x 102 -1.00 x 102 1.20 х 10"2 -1.20 x 102 2.00 x 10-2 -2.00 x 102