18. Calculate the pH of the solution formed when 12.0g of sodium fluoride (0.286mol) (NaF, FW- 41.99 is added to 500.ml of an 0.500M solution of hydrofluoric acid (HF). We start off with a weak acid in solution. When we add the salt of its conjugate base, we make a buffer solution, and the Na" is a spectator ion: The pka for HF is 6.4 x 10 (Acid]-0.500M nase -(Base] = Vaotn mol 0.286mol 12.0g x - 0.286mol 500.x 10-L - 0.572 M 41.99g K (64 x 10) Complete the problem by calculating the pH of the buffer solution.

18. Calculate the pH of the solution formed when 12.0g of sodium fluoride (0.286mol) (NaF, FW- 41.99 is added to 500.ml of an 0.500M solution of hydrofluoric acid (HF). We start off with a weak acid in solution. When we add the salt of its conjugate base, we make a buffer solution, and the Na" is a spectator ion: The pka for HF is 6.4 x 10 (Acid]-0.500M nase -(Base] = Vaotn mol 0.286mol 12.0g x - 0.286mol 500.x 10-L - 0.572 M 41.99g K (64 x 10) Complete the problem by calculating the pH of the buffer solution.

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter16: Acids And Bases

Section: Chapter Questions

Problem 10ALQ

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The hydrogen phthalate ion, C8HsO4, is a weak acid with Ka = 3.91 106. C8H5O4(aq)+H2O(l)C8H4O42(aq)+H3O+(aq) What is the pH of a 0.050 M solution of potassium hydrogen phthalate. KC8H5O4? Note: To find the pH for a solution of the anion, we must take into account that the ion is amphiprotic. It can be shown that, for most cases of amphiprotic ions, the H3O+ concentration is [H3O+]=Ka1Ka2 For phthalic acid, C8H6O4 is Ka1 is 1.12 103, and Ka2 is 3.91 106.
1.56 g of sodium acetate, NaCH;CO, has been 0.20 M ammonia, NH3, and 0.20 M ammonium 4. What is the pH of 0.15 M acetic acid to which 3. What is the pH of a solution that consists of aqueous solution of NH3? the same when you (c) add solid NaCl to a dilute aqueous solution of (b) add solid sodium acetate to a dilute a (a) add solid ammonium chloride to a dilute 1. Does the pH of the solution increase, decrease, or 17.1 and 17.2.) stay solution of acetic acid? aqueous NaOH? 2 Does the pH of the solution increase, decrease, or stay the same when you (a) add solid sodium oxalate, Na,C,O4, to 50.0 mL of 0.015 M oxalic acid, H,C,O4? (b) add solid ammonium chloride to 75 mL of 0.016 M HCl? (c) add 20.0 acetate, NaCH;CO2? of NaCl to 1.0 L of 0.10 M sodium *What is the pH of a solution that consists of chloride, NH4CI? added?
A buffer system is prepared by combining 0.603 moles of ammonium chloride (NH4CI) and 0.713 moles of ammonia (NH3). What will the solution pH be if 0.239 moles of the nitric acid (HNO3) is added to the solution. Nitric acid is a strong acid. The K₁ of ammonia is 1.8 x 10-5. (Two decimal places)
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)?
You are studying a clear solution and you added the pH indicator methyl violet. The colour range of the indicator methyl violet in a clear solution when changing from acidic to basic is yellow (pH 0) to blue purple (pH 1) to violet (pH 2). You initial pH of the solution when tested with a pH meter is O.2. You are going to add 250 drops of 0.1 M HCI. Please select the most appropriate answers to the following two questions. What is the initial colour of the solution at pH 0.2? What is the colour of the solution and what will the pH be after the addition of the HCI? Select 2 correct answer(s) The colour of the solution after the addition of HCI will be clear and the pH will be less than 0.2. The colour of the solution after the addition of HCI will be violet and the pH will be higher than 0.2.
Consider the buffer system of carbonic acid (H₂CO₂) and its salt, KHCO₂, which provides the conjugate base, HCO,. H_COjlog) + HJO W 7 HyO" loạ) + HCOy loa) How does the buffer react when some base is added? The bicarbonate ion (HCO) of the buffer reacts with the base. OHCO and H₂CO, both react with the base. O The buffer does not react. O The carbonic acid (H₂CO₂) of the buffer reacts with the base Question 15 Indicate whether each of the following reactions is an example of reaction of an acid with a metal, reaction of an acid with a carbonate, or acid-base neutralization reaction using the dropdown on the right. Reaction A: ZnCO3(s) + 2HBr(aq) → ZnBr₂(aq) + CO₂(g) + H₂O(l) Reaction B: Zn(s) + 2HCl(aq) → ZnCl₂(aq) + H₂(g) HCI(g) + NaHCO3(s)→ NaCl(aq) + CO₂(g) + H₂O(0) H₂SO4(aq) + Mg(OH)2(s)→ MgSO4(aq) + 2H₂O(1) 3LIOH(aq) + H₂PO₂(aq) → Li₂PO₂(aq) + 3H₂O(0) Cal(s) + H₂SO4(aq) → H₂(g) + CaSO₂(aq) Reaction C: Reaction D: Reaction E: Reaction E
If a buffer solution is made from 300.0 mL of 2.2 M pyridine salt mixed with 350.0 mL of 2.0 M pyridine (see below for skeletal formulas of each), calculate the following: The initial pH of the buffer solution. The pH of the solution if 10.0 mL of 0.400 M HBr is added to the buffered solution. The pH of the solution if 10.0 mL of 0.400 M KOH is added to the buffered solution.
An acid-base equilibrium system is created by dissolving 0.50 mol CH3CO2H in water to a volume of 1.0 L. What is the effect of adding 0.50 mol CH3CO2–(aq) to this solution? 1.The pH of the solution will equal 7.00 because equal concentrations of a weak acid and its conjugate base are present. 2.Some CH3CO2H(aq) will ionize, increasing the concentration of CH3CO2–(aq) and increasing the pH.3.Some CH3CO2–(aq) will react with H3O+, increasing the concentration of CH3CO2H(aq) and reestablishing the solution equilibrium. b. 2 only c. 3 only d. 1 and 3 e. 1, 2, and 3
ACID-BASE EQUILIBRIA Doc Jill wants to determine the Ao of a weak acid she isolated called Xcitingpartic acid (HXp). She prepared a solution of the weak acid by diluting 2.7 ml of 0.20 M HXp with 19.3 mlL of water. Upon measuring the conductivity of the solution and a blank, she obtained 205.0 µS/cm and 2.0 uS/cm, respectively. She also measured the pH of the solution and got a pH of 3.49. Help her find the following: 1. Concentration of the weak acid (HXp) after dilution 2. Corrected conductivity 3. Molar conductivity of the solution 4. Equilibrium concentration of H30, and Xp 5. a 6. Equilibrium concentration of the weak acid (HXp) 7. K, 8. Ao
5 A buffer system is prepared by combining 0.569 moles of ammonium chloride (NH4Cl) and 0.586 moles of ammonia (NH3). What will the solution pH be if 0.158 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 105. (Two decimal places) Type your answer..... Submit
11.An acid-base equilibrium system is created by dissolving 0.20mol CH3COOH in water and diluting the resulting solution to a volume of 1.0 L. What is the effect of adding 0.020 mol CH3COO (aq) to this solution? How will pH change (calculate pH before and after the addition. Ka of CH3COOH is 1.76 x10-5)? How will concentrations of CH3COOH and CH3COO at equilibrium change?
A 0.018 M solution of salicylic acid, HOC6H4CO2H, has the same pH as 0.0038 M HNO3solution. (a) Write an equation for the ionization of salicylic acid in aqueous solution. (Assume only the –CO2H portion of the molecule ionizes.) (b) What is the pH of solution containing 0.018 M salicylic acid? (c) Calculate the Ka of salicylic acid.

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