Answered: Calculate the pH of a solution prepared…

Calculate the pH of a solution prepared by dissolving 0.040 moles of sodium nitrite (NaNO2) in 200 mL of a 0.10 M nitrous acid solution (HNO2, Ka = 5.1 x 10-4).

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter13: Acids And Bases

Section: Chapter Questions

Problem 31QAP: What is the pH of a solution obtained by adding 13.0 g of NaOH to 795 mL of a 0.200 M solution of...

See similar textbooks

Related questions

Q: What is the pH of a solution that contains 0.1 M benzoic acid and 0.4 M potassium benzoate? The Ka…

A: Since on dissolving in water benzoic acid give below reaction benzoic acid -------> benzoate ion…

Q: What is the pH of a 3.50 M solution of NH4CI (Ká of NH3= 1.8 x 105)?

Q: What is the pH of a solution prepared by dissolving 1.00 g of the weak acid HA (molar mass = 138.95…

A: pH of solution can be found using the henderson-hesselbech equation.

Q: Acids, Bases, Hydrolysis, Buffers, Titrations 1. Calculate the pH and percent ionization for 0.50 M…

Q: 1. Consider a solution of NaHA for which F = 0.050 mol L¹, K₁1 = 4.70 x 10³ and K₁2 = 1.80 x 10-10,…

Q: Calculate the pH of a 0.86 M solution of a weak base CH3NH2 (Kb = 1.8 x 10-5) Write a chemical…

Q: What is the pH of a solution that contains 0.15 M benzoic acid and 0.45 M potassium benzoate? The Ka…

A: Assuming benzoic acid dissolves in water and produces y concentration of ions Since the reaction is…

Q: Vhat is the pH of a solution containing 0.2 M citric acid (pKa = 5.4) and 0.1 M sodium citrate?

A: Introduction: Since having sodium citrate that is a buffer solution so we can use the…

Q: What is the pH of a 0.0270 M solution of hydrocyanic acid, HCN (Ka = 4.9 × 10⁻¹⁰)?

A: HCN is a weak acid , it ionizes as follows HCN <----> H+ + CN- Given , Concentration of HCN…

Q: Calculate the pH of a solution that is prepared by dissolving 7.85 g of lactic acid (90.08 g/mol)…

A: Here we are required to find the pH of solution prepared by mixing lactic acid and sodium lactate.

Q: Would you expect a solution of ammonium chloride (NH4Cl) to be acidic or basic when added to water?…

A: Introduction- For the salts of strong acids and strong bases, the pH of salt will be neutral that is…

Q: 5.Calculate the pH of a 1.0 x 10^-4 M of NaCN. *

A: Given: [NaCN] = 1.0 x 10-4 M Ka of HCN = 6.2 x 10-10 Kw = 1.0 x 10-14

Q: Calculate the pH of a 1.0 x 10^-4 M of NaCN

Q: What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M methylamine, CH 3NH 2, with 25.00…

Q: 2. Calculate the pH of a 1.0 x 10-4 M of NaCN

Q: 10. Calculate the pH of a 0.150M solution of sodium acetate (NaC,H,O;) at 25°C. (K, for acetic acid…

A: Given-> Concentration of sodium acetate = 0.150 M Ka (CH3COOH) = 1.8 × 10-5

Q: Suppose that ammonia, applied to a field as a fertilizer, is washed into a farm pond containing 3.0…

Q: What is the pH of an aqueous solution of 1.45×10-2 M nitric acid?

A: Nitric acid i.e HNO3 is a strong acid. Hence it dissociates into ions completely as per the…

Q: Calculate the number of moles of HF that must be present in 500 mL of solution to give a pH of 3.5.…

Q: Calculate the pH of a solution that is made by combining 55 mL of 0.060 M hydrofluoric acid with 125…

A: A mixture of HF and NaF forms an acidic buffer and its pH is given by pH of the acidic buffer = pKa…

Q: The PH of 0.0296M HA ( Ka 8.4 *10-9) plus * . . 0.1026 M NaA is 4.3 2 O 8.6 7.5 O

A: The question is based on the concept of PH calculations. we have been given a weak acid and its…

Q: 1. Calculate the pH of a 200.0-mL solution containing 0.050 M benzoic acid (C6H5COOH) and 0.025 M…

A: pH = pKa + log[C6H5COO-]/[C6H5COOH]

Q: Calculate the pH in the solution formed by adding 10.0 mL of 0.050 M NaOH to 40.0 mL of 0.0250 M…

A: The number of moles of benzoic acid and NaOH in the solution can be calculated using equation (1),

Q: What is the pH of a solution when 2. 75 g of ammonium chloride, NH4CI, is used to make 100 cm3 of…

A: Number of Mole-ratio of given mass of substance to the molar mass of substance is called number of…

Q: Calculate the pH and percent ionization of 0.150 M ascorbic acid K31 = 7.9x 10-5 ascorbic acid,…

Q: What is the pH of a solution prepared by dissolving 1.00 g of the weak acid HA (molar mass = 138.95…

Q: What is the pH of a 0.0650 M solution of hydrocyanic acid, HCN (Ka = 4.9 × 10⁻¹⁰)?

Q: What is the pH of a solution that is 0.28 M in acetic acid, HC2H3O2, and 0.69 M in sodium acetate,…

A: Answer:- This question is answered by using the simple concept of calculation of pH of a solution…

Q: What is the pH of a solution prepared by dissolving 1.00 g of the weak acid HA (molar mass = 138.95…

Q: find the pH of the solution Ca (OH) 2, which is obtained when dissolving 0.5 grams of Ca (OH) 2 in 1…

A: We can find the concentration of Calcium hydroxide using moles and volume. Then we know we have…

Q: What is the pH of a 0.300 M solution of aniline (CH NH, Kb = 4.3 x 10)?

A: The pH scale is given by the scientist Sorensen in order to express the [H3O+] ion of a solution. It…

Q: When 2.0 x 10-2 mole of nicotinic acid (a monoprotic acid) is dissolved in 350. mL of water, the pH…

A: Nicotine is a weak monoprotic acid so it dissociated in less amount. So we can denotes it by HA .

Q: Determine the pH at 25C of a solution prepared by dissolving 0.35 mole of ammonium chloride in 1. L…

A: Concentration of ammonia Volume of ammonia solution Number of moles of ammonium chloride added =…

Q: A solution of acetic acid was prepared from the mixture of 200 ml of [CH3COOH] 0.500 mol L-1 in 300…

Q: Calculate the pH of the solution formed when 45.0 mL of 0.100 M NaOH is added to 50.0 mL of 0.100 M…

A: NaOH will react completely with acid CH3COOH as its a strong base NaOH + CH3COOH -------->…

Q: What is the pH of a 0.0100 M solution of analine (C6H5NH2) , a weak base. Kb= 4.0 x10-10

A: The chemical equation for aniline can be written as: This equation shows that aniline is a base,…

Q: Calculate the pH of a 0.424 M aqueous solution of hydrocyanic acid (HCN, Ka = 4.0×10-10).

A: pH of the solution can be calculated by using the formula, pH = [H+]. Given data, Concentration of…

Q: Fill in the blanks: Ka of acetic acid is 1.80 x105 and that for hypochlorous acid is 3.0 x 108 The…

Q: Solutions of sodium salts of the acids in the following table are prepared with an initial…

A: Dissociation of a weak acid is given by: HA ⇌ H+ + A- The acid dissociation constant of this…

Q: how you determine the pH when 15 ml of 0.100 M HCI is ado 080 M NH3 (K, = 1.6 x 10-6)

A: Given, Kb = 1.6×10-6 pKb = -log(Kb) = -log(1.6×10-6) = 5.82 Molarity of HCl = 0.100 M Volume of HCl…

Q: |Calculate the pH of a 7.2 × 10 ´ M aqueous solution of aluminum chloride, AIC13. The acid…

A: pH - pH is defined as negative logarithm to the base 10 of H+ ion concentration. Or pH can also be…

Q: 2. Calculate the pH of a solution containing 0.75 M lactic acid, HC3H5O3, (Keq= 1.4 x 104) and 0.25M…

A: The solution contains a mixture of 0.75 M lactic acid and 0.25 M sodium lactate.

Q: What is the pH of a 0.0500 M solution of hydrocyanic acid, HCN (Ka = 4.9 × 10⁻¹⁰)?

A: Given -> Molarity of HCN = 0.0500 M Ka = 4.9 × 10-10

Q: what is the ph of 0.0349 M anilinium hydrochloride (C6H5NH3CI) solution in water, given that K for…

Q: The Ka of hypobromous acid, HOBr, is 2.6 x 10-9. Calculate the pH of a solu tion which is composed…

A: PH of acidic buffer can be calculated as follows

Q: HCIO is a weak acid (K. = 4.0 x 10-8) and so the salt NaCIO acts as a weak base. What is the pH of a…

Q: HCIO is a weak acid (K, = 4.0 x 10-8) and so the salt NaCIO acts as a weak base. What is the pH of a…

A: pH = 7 +12 (pka + log c)

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

100%

Calculate the pH of a solution prepared by dissolving 0.040 moles of sodium nitrite (NaNO₂) in 200 mL of a 0.10 M nitrous acid solution (HNO₂, Ka = 5.1 x 10^-4).

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Step 5

Step by step

Solved in 5 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

What is the pH of a solution obtained by adding 13.0 g of NaOH to 795 mL of a 0.200 M solution of Sr(OH)2? Assume no volume change after NaOH is added.
Lactic acid, C3H6O3, occurs in sour milk as a result of the metabolism of certain bacteria. Calculate the pH of a solution of 56. mg lactic acid in 250. mL water. Ka for D-lactic acid is 1.5 × 10−4.
8. (a) Calculate the percent ionization of a 0.20 M solution of the monoprotic acetylsalicylic acid (aspirin) for which Ka = 3.0 x 10-4 .(b)The pH of gastric juice in the stomach of a certain individual is 1.00. After a few aspirin tablets have been swallowed, the concentration of acetylsalicylic acid in the stomach is 0.20M. Calculate the % ionization of the acid under these conditions. What effect does the nonionized acid have on the membranes lining of the stomach? 9. Calculate the [H+], [C2O4-2], and [H2C2O4] in a 0.0010M H2C2O4 solution. (Ka = 5.4 x 10-2)
Calculate the pH of the solution formed when 45.0 mL of 0.100 M NaOH is added to 50.0 mL of 0.100 M CH3COOH(Ka = 1.8 x 10-5).
Calculate the pH of a 0.65 M solution of aqueous bromous acid (HBrO2, Ka = 1.2 x 10-5).
How many grams of potassium lactate (C3H5O3K) need to be dissolved in 129 mL of a 1.71 M lactic acid (HC3H5O3, Ka = 1.4 × 10−4) solution, so that the pH of the solution is 4.22? Report your answer to THREE significant figures.
(a) Calculate the percent ionization of a 0.20 M solution of monoprotic acetylsalicylic acid (aspirin) for which Ka = 3.0 x 10^-4. (b) The pH of gastric acid juice in the stomach of a certain individual is 1.00. After a few aspirin tablets have been swallowed, the concentration of acetylsalicylic acid in the stomach is 0.20 M. Calculate the percent ionization of the acid under these conditions.
Propionic acid, HC3H5O2, has Ka= 1.34 x 10–5. (a) What is the molar concentration of H3O+ in 0.15 M HC3H5O2 and the pH of the solution? (b) What is the Kb value for the propionate ion, C3H5O2–? (c) Calculate the pH of 0.15 M solution of sodium propionate, NaC3H5O2. (d) Calculate the pH of solution that contains 0.12 M HC3H5O2 and 0.25 M NaC3H5O2.
(a) Calculate the acetate ion concentration in a solution prepared by dissolving 8.70×10-3 mol of HCl(g) in 1.00 L of 1.10 M aqueous acetic acid (Ka = 1.80×10-5). (b) Calculate the pH of the above solution. Give your answer to two decimal places.
A solution of acids is made by mixing 0.19 M HNO3 and 0.45 M CH3COOH (Ka (CH3COOH) = 1.8 x 10-5). Calculate the pH of the solution.
10. How many moles of CH;COONA (sodium acetate) must be added to 2.0 L of 0.10 M CH;COOH (acetic acid) to give a solution that has a pH equal to 5.00? Ignore the volume change due to the addition of CH;COONA (sodium acetate). The Ka of CH;COOH = 1.8 x 105. (Note – the Na at the end of the molecule is the same as the Na at the beginning - it just drops off).
(a) Calculate the pH in the solution formed by adding10.0 mL of 0.050 M NaOH to 40.0 mL of 0.0250 M benzoicacid (C6H5COOH, Ka = 6.3 x 10-5). (b) Calculate the pHin the solution formed by adding 10.0 mL of 0.100 M HCl to20.0 mL of 0.100 M NH3.