The pH of an aqueous solution of 0.534 M hydrocyanic acid, (K₁ (HCN) = 4.00 × 10−¹⁰) isaSubmit AnswerUse the References to access important values if needed for this question.Retry Entire Group9 more group attempts remaining

Given:Initial concentration of hydrocyanic acid=0.534 MKa of HCN=4.00x10-10We have to find the pH of…

Answered: The pH of an aqueous solution of 0.534…

The pH of an aqueous solution of 0.534 M hydrocyanic acid, (K₂ (HCN) = 4.00 × 10-¹0) is Submit Answer Retry Entire Group 9 more group attempts remaining

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 57QRT: The pH of a 0.10-M solution of propanoic acid, CH3CH2COOH, a weak organic acid, is measured at...

See similar textbooks

Related questions

Q: 3. A 0.0560 g quantity of acetic acid is dissolved in enough water to make 50.0 mL of solution.…

A: (a) Initial Concentration of CH3COOH Given mass of acetic acid = 0.056 gms, Volume of…

Q: The pH of a chemical solution is given by theformula pH = - log10 [H+ ] where [H+ ] is the…

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…

Q: Calculate the molar H3O* ion concentration of solution that has a pH of (a) 9.21 (b) 0.45 (c) 7.32…

A: pH: It can be defined by saying the power of hydrogen in any compound. It ranges from 0 to 14. We…

Q: (a) Calculate the percent ionization of 0.00310 M butanoic acid (K₂ = 1.5e-05). % ionization = % (b)…

Q: CoHsOH(ag) + H2O0 → CaHsO(aq) + H3O*@g K= 1.12 x 1010 (a) Phenol is a weak acid that partially…

A: Since you have asked a question with multiple parts, we are solving first three parts for you. For…

Q: Given that Ka for acetic acid is 1.8 x 10-5 and that hypochlorous acid is 3.0 x10-8 , which is a…

A: An acid is a species that can donate an H+ ion.The conjugate base of an acid should have one less H…

Q: Determine the pH of each of the following solutions. (a) 0.826 M hydrocyanic acid (HCN) (weak acid…

A: (a) 0.826 M HCN(b) 0.656 M HBrO(c) 0.673 M pyridine

Q: Calculate the pH of a 0.88 M aqueous solution of the base aniline, Ce H; NH2 (K, = 4.0 x 1010). C,H;…

A: Here, we have to calculate the pH of a 0.88 M aqueous solution of the base aniline. Given: Kb for…

Q: Determine the pH of each of the following solutions. (a) 0.246 M hydrocyanic acid (HCN) (weak…

A: In chemistry, pH ( "potential of hydrogen" or "power of hydrogen") is a scale used to specify the…

Q: What is the pH of an aqueous solution of 0.159 M sodium cyanide (NaCN)? (Kb of CN- = 2.5 x 10-5)

A: Given, The concentration of sodium cyanide (NaCN) = 0.159 M Kb for CN- = 2.5 x 10-5. pH is the…

Q: What is the pH of a 0.1250 M CH3NH3Br? Kb for CH3NH2 is 3.70e-4.

A: Given, The pH of a 0.1250 M CH3NH3Br is : Kb for CH3NH2 is 3.70e-4.

Q: Determine the pH of each of the following solutions. (a) 0.526 M hypochlorous acid (weak acid with…

Q: The pH of an aqueous solution of 0.532 M hydrofluoric acid, ( K₂ (HF) = 7.20 × 10¯4) is

A: Concentration of HF solution (C) = 0.532 MKa for HF = 7.20 × 10-4 pH of the solution = ?

Q: Determine the pH of each of the following solutions. (a) 0.762 M hypobromous acid (weak acid…

A: Here, we have to calculate the pH of the given solutions: 0.762 M hypobromous acid (weak acid with…

Q: The lactate ion, C,H,O7 (aq), reacts with water to form lactic acid and hydroxide ion. C,H;05 (aq) +…

A: Given : [OH-] = 5.2 x 10-6 M So as per ICE table x = 5.2 x 10-6 M

Q: Determine the pH of each of the following solutions. (a) 0.112 M acetic acid (weak acid with Ka…

A: pH : It is scale which measures the acidity or basicity of the solution under observation. If pH…

Q: Determine the pH of each of the following solutions. (a) 0.549 M hydrogen peroxide (weak acid with…

Q: Determine the pH of each of the following solutions. (a) 0.684 M hypochlorous acid (weak acid…

Q: Determine the pH of each of the following solutions. (a) 0.134 M hypochlorous acid (weak acid with…

A: The objective of the question is to calculate the pH of three different solutions, each containing a…

Q: The pH of an aqueous solution of 0.0655 M ammonium bromide, NH4 Br(aq), is (Assume that K, (NH3) =…

A: The question is based on the concept of the pH of the solution.It is defined as a negative logarithm…

Q: (a) Calculate the percent ionization of 0.00190 M hypochlorous acid (K₂ = 3e-08). % ionization = %…

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

Q: THE X IS SMALL APPROXIMATION The initial concentration and Ka of several weak acid (HA) solutions…

Q: Q3. This question is about the pH of several solutions. Give all values of pH to 2 decimal places.…

A: PH of solution determines the nature of solution whether it is acid or basic solution. The acidic…

Q: Calculate the pH of a solution containing 0.20 M CH3COOH and 0.30 M CH;COONA. [Ka CH3COOH = 1.8 x…

Q: The pH of an aqueous solution of 0.175 M ammonium iodide, NH¼I (aq), is This solution is

A: Given : Concentration of NH4I = 0.175 M Since NH4I is made up of weak base NH3 and strong acid HI.…

Q: a) Write the formula for the conjugate base of HPO, -2 b) Write the formula for the conjugate acid…

Q: the pH and concentrations of species the following sõlutions (a) 0.20 M K,HPO4 An amphiprotic…

A: Amphiprotic species Amphiprotic species can act both as acid and base by donating or accepting…

Q: The pH of a 1.00 M Solution -1 of Nitrous acid HNO2 (pKb =10.6) is

A: HNO2 is a weak acid. pH of 1M solution need to be found out here. Dissociation of this weak acid in…

Q: Calculate the pH of each of the following solutions. (a) 0.109 M HONH, (Kb = 1.1 × 10-8) 4.0 9.34 x…

A: The concentration of HONH2 = 0.109 M The concentration of HONH3+ = 0.109 M

Q: Determine the pH of each of the following solutions. (a) 0.257 M hypobromous acid (weak acid with…

Q: Determine the pH of each of the following solutions.

A: Given : concentration of weak acid and base. tip : pH = -log[H+]

Q: 02-11 Tobiem 2.13] A solution has an H+ concentration of 10-5 M. (a) What is the pH of this…

Q: What is the concentration of hydroxide ion in a 0.170 M aqueous solution of hydroxylamine, NH2OH?…

A: pH of solution is defined as negative logarithm of hydrogen ions concentration.

Q: (a) 33. Which one of the following statements regarding acid-base property is NOT correct? pH + pOH…

Q: Calculate the pH of 0.5 mol/L sodium hydrogen carbonate, NaHCO3. The Ka,1 of carbonic acid, H₂CO3,…

Q: Rank the following aqueous solutions in terms of pH. Why Are they in that order? (a)0.1 M CH3COOH…

Q: (a) Calculate the percent ionization of 0.00800 M butanoic acid (K, = 1.5e-05). % ionization = % (b)…

A: Percent ionization

Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

The pH of an aqueous solution of 0.534 M hydrocyanic acid, (K₁ (HCN) = 4.00 × 10−¹⁰) is
a
Submit Answer
Use the References to access important values if needed for this question.
Retry Entire Group
9 more group attempts remaining

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: Introduce the given problem

VIEW

Step 2: Calculate concentration of H+

VIEW

Step 3: Calculate pH

VIEW

Solution

VIEW

Step by step

Solved in 4 steps with 4 images

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

Assuming that the conductivity of an acid solution is proportional to the concentration of H3O+, sketch plots of conductivity versus concentration for HCl and HF over the 0- to 0.020 M concentration range.
A student is asked to bubble enough ammonia gas through water to make 4.00 L of an aqueous ammonia solution with a pH of 11.55. What volume of ammonia gas at 25C and 1.00 atm pressure is necessary?
The sec-butyl cation can react as both a Brnsted-Lowry acid (a proton donor) and a Lewis acid (an electron pair acceptor) in the presence of a watersulfuric acid mixture. In each case, however, the product is different. The two reactions are as follows: (a) In which reaction(s) does this cation react as a Lewis acid? In which reaction(s) does it react as a Brnsted-Lowry acid? (b) Write Lewis structures for reactants and products and show by the use of curved arrows how each reaction occurs.
Place the species in each of the following groups in order of increasing acid strength. a. H2O, H2S, H2Se (bond energies: HO, 467 kJ/mol; HS, 363 kJ/mol; HSe, 276 kJ/mol) b. CH3CO2H, FCH2CO2H, F2CHCO2H, F3CCO2H c. NH4+, HONH3+ d. NH4+, PH4+ (bond energies: NH, 391 kJ/mol; PH, 322 kJ/mol) Give reasons for the orders you chose.
Rank the compounds in each of the following groups in order of increasing acidity or basicity, as indicated, and explain the order you assign. (a) acidity: HCI, HBr, HI. (b)basicity: H2O, OH-, H-, CI-. (c) basicity: Mg(OH)2, Si(OH)4, ClO3(OH) (Hint: Formula could also be written as HCIO4). (d) acidity: HF, H2O, NH3, CH4
The pH of a 0.10-M solution of propanoic acid, CH3CH2COOH, a weak organic acid, is measured at equilibrium and found to be 2.93 at 25 °C. Calculate the Ka of propanoic acid.
Follow the directions of Question 65 for the following bases: (a) SO32- (b) CHO2- (c) NO2-
Consider the following data on some weak acIas and weak bases: acid base K, Kb name formula name formula 8. acetic acid HCH;CO2|1.8 × 10 hydroxylamine HONH, |1.1 × 10° HNO2 ethylamine C,H,NH2 6.4 x 10 nitrous acid 4.5 x 10 Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. solution pH 0.1 М КCН3СО2 choose one 0.1 M C2H5NH3BR choose one 0.1 M NaNO3 choose one 0.1 M NaNO2 choose one
The pH of an aqueous solution of 0.0917 M ammonium perchlorate, NH4ClO4 (aq), is Kb (NH3) = 1.80 × 10-5.) This solution is Submit Answe acidic basic neutral Entire Group 9 more group attempts remaining (Assume that
Consider the following data on some weak acids and weak bases: acid base Bo Ka K, name formula name formula acetic acid HCH,CO, 1.8 × 10 -, methylamine CH;NH, 4.4 x 10 -4 HNO, 4.5 x 10 4 ethylamine C,H,NH, 6.4 x 10 * -4 nitrous acid Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have t the solution that will have the next lowest pH, and so on. solution pH 0.1 M CH3NH3CI choose one v 0.1 M NANO2 choose one v 0.1 M KCH3CO2 choose one v 0.1 M C2H5NH3Br choose one v Explanation Check O 2022 McGraw Hill LLC. All Rights Reserved. T 回 0中g W DELL
Subject:
1) A conjugate acid is defined as 2) In the general ionization reaction: HX(aq) + H,0(1) = H,0* + X(aq)', water acts as a base or as an acid? 3) An aqueous solution with pOH 8.0 is acidic or basic?, 4) Which is the conjugate base of this acid?: HNO; (Use the appropriate ionic charge) 5) Mention a salt that is pH neutral