Answered: Calculate the pH of a 0.10 M acid…

Science

Chemistry

Calculate the pH of a 0.10 M acid H2ASO4 if its Ka = 5.6 x 10ˉ⁸?

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

Section14.7: Problem Solving Using Ka And Kb

Problem 14.19E

See similar textbooks

Related questions

Q: HClO is a weak acid (Ka = 4.0 × 10–8) and so the salt NaClO acts as a weak base. What is the pH of a…

A: Ka of HClO is given as 4 x 10-8. It is required to calculate the pH of solution that is 0.054M in…

Q: The CO2 we breathe reacts with water in our blood to form the weak acid H2CO3. What mole ratio of…

A: Given:Ka of H2CO3 is 4.4 ✕ 10−8

Q: Calculate the pH of a 0.84 M HONH2 solution. Give your answer to three sig figs. Kb(HONH2) = 1.0 x…

A: Given: The concentration of HONH2 solution = 0.84 M Kb(HONH2) = 1.0 x 10‒5 To Calculate: pH of the…

Q: If the Kb for hydrazine, N2H4(aq), is 1.7 x 10-6 , calculate the pH of a 1.8 mol/L solution of…

A: To calculate the pH of a 1.8 mol/L solution of hydrazine. Given: Kb for hydrazine, N2H4(aq) = 1.7 x…

Q: For H2CO3, Ka1 = 4.3 × 10–7, Ka2 = 4.7 × 10–11. What is the pH of a 0.36 M solution of carbonic…

A: We have to predict the pH of 0.36 M of carbonic acid .

Q: Household bleach is prepared by dissolving chlorine in water. Cl2 (g) + H2O « H+ (aq) + Cl-…

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: a) Label each species as an Bronsted-Lowry acid or base. Show the conjugate acid-base pairs. HCO; +…

Q: What is the pH of a 0.82 M HClO, hypochlorous acid solution, which has a Ka of 3.2 × 10–8 at 25°C?

Q: Calculate the pH of a .10 M solution of formic acid (HCHO2). The Ka of formic acid is 1.8 x 10-4.

Q: Perform the following to determine the pH of a lactic acid solution. Write the acid/base reaction…

A: pH is negative logarithm of the hydronium ion concentration in a solution. Its value ranges from…

Q: The compound methylamine is a weak base like ammonia. A solution contains 0.199 M CH3NH3* and 0.117…

A: TThe base is the substance that gives OH- or accepts H+ ions in solution. The Henderson Hasselbalch…

Q: Is H2Cr2O2 an acid, base, or neutral? please justify your answer with an equation showing its…

A: The question is based on the concept of chemical substances we need to identify the nature of the…

Q: Calculate the pH of 0.0037M solution of H2CO, given that K,1- 4.3 x 10 and Kz = 5.6 x 1011

Q: What will be the pH of a solution containing 0.200 M NaH2PO4 and 0.200 M Na2HPO4? Ka(NaH2PO4) = 6.2…

A: Given, Molar concentration of weak acid, NaH2PO4 or H2PO4- = [H2PO4-] = 0.200 M Molar concentration…

Q: Hydrazine, N2H4, is used as a rocket fuel, but also as a reactant in organic chemistry. The K of…

Q: If a solution of HF (Ka = 6.8 x 10-4) has a pH of 3.65, calculatethe concentration of hydrofluoric…

A: The term pH of the solution is a measure of the acidity or the basicity of a given solution. More…

Q: Methylammonium halides, like CH3NH3CI (67.52 g.mol), are white or light colored powders used…

A: CH3NH3Cl is salt of a weak base CH3NH2 and strong acid HCl. Therefore, the hydrolysis reaction of…

Q: 10. Calculate the pH of a solution of CH3NH2(aq) Methylamine, K = 4.3x10 that has an initial…

A: Information of question

Q: Hydrazine, N2H4, has Kb = 1.3E-6. Calculate the pH of a 0.644 M solution of N2H4.

Q: Which describes a solution whose [H3O]* concentration is 3.72 x 105 M? acidic solution, pH = 4.429…

A: Given, [H3O+] = 3.72 x 10-5 M PH is defined as negative logarithm of concentration of Hydronium…

Q: What is the pH of a 0.20 M solution of CH3NH3NO3 at 25 °C? At this temperature, the K₁ for CH3NH2 is…

A: Given:Given is a solution of CH3NH3NO3Concentration of solution = Temperature = 25oCThe pH of a…

Q: What is the pH of a solution that is 0.0530 M in NaClO at 25 °C? The Ka for HClO is 4.0×10−8

A: Given thatConcentration of NaClO = [ClO–] = 0.0530 MKa for HClO = 4.0×10−8Kb for ClO– =

Q: Calculate the pH of a 0.600 M solution of methylamine CH3NH2. Kb = 4.4 x 10–4

A: CH3NH2 is a base and CH3NH3+ is its conjugated acid. pKb of CH3NH2 is 4.4×10-4. Expression for Kb is…

Q: HClO is a weak acid (Ka = 4.0 × 10–8) and so the salt NaClO acts as a weak base. What is the pH of a…

A: It is required to calculate the pH of the solution that is 0.016 M in NaClO.Ka for HClO = 4 x 10-8…

Q: What is the pH of a solution prepared by dissolving 0.450 mol of NH3 in sufficient water to make…

A: Given, The pH of a solution prepared by dissolving 0.450 mol of NH3 in sufficient water to make…

Q: Calculate the pH of a 0.597 M solution of chloroacetic acid (CICH;CO,H, K, = 1.36 x 10-3).

Q: For H2CO3, Ka1 = 4.3 x 10 7, Ka2 = 4.7 × 10 11. What is the pH of a 0.11 M solution of carbonic…

Q: f) Calculate the pH of the following solutions: (i) A 0.045 M solution of sulphuric acid. (ii) A…

Q: Lactic acid, HC3H5O3, is a weak acid; write an equation for its ionization in aqueous solution. If…

A: given Lactic acid, using PH calculate the value of H+ , apply the H+=Cα using the alpha value…

Q: Formic acid, HCOOH, has Ka= 1.8 x 10–4. Calculate the molar concentration of H3O+ in 0.15 M HCOOH…

A: using given value of ka and concentration use equaction- H+=cα α=kaC use this boh calculate the…

Q: Calculate

A: Option c is correct answer. pH= 10.11

Q: What is the pH of a 0.844 M solution of hypochlorous acid (Ka 2.9 x 10-8)?

Q: Determine the pH of a 0.15 M solution of Ca(BrO2)2 at 25 °C. At the same temperature, Ka for HBRO, =…

Q: The active ingredient of bleach such as Clorox is sodium hypochlorite (NaClO). Its conjugate acid,…

A: Given:The word pH stands for the potency of hydrogen and it is used to measure the concentration of…

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

2. Calculate the pH of a 0.10 M acid H2ASO4 if its Ka = 5.6 x 10ˉ⁸?

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

VIEW

Step 2

VIEW

Step 3

VIEW

Step by step

Solved in 3 steps with 3 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

For H2CO3, Ka1 = 4.3 × 10–7, Ka2 = 4.7 × 10–11. What is the pH of a 0.36 M solution of carbonic acid?
Calculate the pH of a 0.597 M solution of chloroacetic acid (CICH;CO,H, K, = 1.36 x 10³).
The CO2 we breathe reacts with water in our blood to form the weak acid H2CO3. What mole ratio of H2CO3/HCO3− is required to obtain a pH of 7.40, the pH of blood? (Assume that the Ka of H2CO3 is 4.4 ✕ 10−8.)
Determine the pH of a 0.15 M solution of Ca(BrO2)2 at 25 °C. At the same temperature, Ka for HBRO2 = 5.6 x 10 and K, for Ca(OH)2 > 1.
HClO is a weak acid (Ka = 4.0 × 10–8) and so the salt NaClO acts as a weak base. What is the pH of a solution that is 0.054 M in NaClO at 25 °C?
Calculate the pH of a 0.600 M solution of methylamine CH3NH2. Kb = 4.4 x 10–4
If a solution of HF (Ka = 6.8 x 10-4) has a pH of 3.65, calculatethe concentration of hydrofluoric acid.
Household bleach is prepared by dissolving chlorine in water. Cl2 (g) + H2O « H+ (aq) + Cl- (aq) + HOCl Ka for HOCl is 3.2 x10-8 . How much chlorine must be dissolved in one liter of water so that the pH of the solution is 1.19? Caproic acid HC6H11O2 is found in coconut oil and is used in making artificial flavors. A solution is made by dissolving 0.450mol of caproic acid in enough water to make 2.0L of solution. The solution has [H+] 1.7 x 10-3 M. what is Ka for caproic acid? Phenol, once known as carbolic acid, HC6H5O, is a weak acid. It was one of the first antiseptics used by Lister. Its Ka is 1.1 x 10-10. A solution of phenol is prepared by dissolving 14.5g of phenol in enough water to make 892mL of solution. For this solution, calculate the pH HC3H5O3, is found in sour milk. What is the pH of 0.30M lactic acid? Ka=1.4 ' 10-4
Lactic acid, HC3H5O3, is a weak acid; write an equation for its ionization in aqueous solution. If 0.15 M solution of lactic acid has pH = 2.34, calculate the molar concentration of H3O+in the solution. What are the Ka of lactic acid and the degree of ionization of the acid?
Hydrazine, N₂H4, is used as a rocket fuel, but also as a reactant in organic chemistry. The K, of hydrazine is 9.1 x 107. If 2.50 × 103 mol of hydrazine are added to water to make up 0.550 L of solution, what is the pH of the solution? Select the correct answer below: ○ 8.8 O9.1 9.3 ○ 9.8
The [H3O+] of Coca-Cola Classic ® is 3.2 x 10-3. What is its pH? Is it acidic or basic?
Perform the following to determine the pH of a lactic acid solution. Write the acid/base reaction between lactic acid, HC3H5O3 and water. Write an equilibrium expression for the reaction between lactic acid and water. If the Ka of lactic acid is 3.18 x 10-4, what is the pH of a 0.500 M solution of lactic acid?