The acid dissociation constant \( K_a \) of carbonic acid \((\text{H}_2\text{CO}_3)\) is \(4.5 \times 10^{-7}\).Calculate the pH of a \(1.6 \, \text{M}\) solution of carbonic acid. Round your answer to 1 decimal place.**Input Field:**pH = [ ]**Buttons:**- Clear (X)- Undo (⟲)- Help (?)

Given : Concentration of H2CO3 = 1.6 M And Ka (first dissociation) of H2CO3 = 4.5 X 10-7 The first…

Answered: The acid dissociation constant K of…

The acid dissociation constant K of carbonic acid (H,CO, is 4.5 × 10¯'. Calculate the pH of a 1.6 M solution of carbonic acid. Round your answer to 1 decimal place. pH

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: -7 The acid dissociation constant K, of alloxanic acid (HC,H,N,O,) is 2.24 x 10'. Calculate the pH…

Q: The concentration of the hydrogen ions in an aqueous solution is 1.7 x 10-11. Determine the pH. Use…

A: Given [H+] = 1.7*10-11

Q: The pHpH scale for acidity is defined by pH=−log[H+]pH=-log[H+] where [H+][H+] is the concentration…

A: pH scale for acidity is defined by pH= −log [H+], where [H+] is the concentration of hydrogen ions…

Q: The pH of a 0.54M solution of boric acid (HBO3) is measured to be 4.75. Calculate the acid…

Q: (i) Define pH in words. The strong acid HClaq has a pH value of 1, use the following equation for a…

A: pH is the power of a substance that how much acidic or alkaline that substance is.

Q: Give the definitions of pH and pKa. What are the differences between these two terms? Calculate the…

A: pH-: The negative logarithm of hydrogen ion concentration in moles per liter in an aqueous solution…

Q: Determine the pH of a solution that is 0.25 M CH3COOH and 0.15 M CH3COONa. Be sure your answer has…

Q: A chemist dissolves 700. mg of pure sodium hydroxide in enough water to make up 60. mL of solution.…

A: The objective of this question is to calculate the pH of a solution of sodium hydroxide (NaOH) that…

Q: The concentration of hydroxylamine in a solution is 0.71 M. What is the pH of the solution? The Kb…

A: Given :- [HONH2] = 0.71 M Kb for HONH2 = 1.1 × 10-8 To calculate :- pH of solution

Q: The equilibrium expression for any weak acid can be written as HA (aq) + H2O (1) = A- (aq) + H3O+…

A: The equilibrium constant of a chemical reaction at equilibrium is defined as the ratio of the…

Q: 1. S)A student prepares a solution of 23.25 g of acetic acid dissolved in enough water to make 2.00…

A: Given, CH3COOH (aq) + H2O (l) ⇌ H3O+ (aq) + CH3COO-(aq) mass of acetic acid = 23.25 g Volume of the…

Q: 10.T/ An industrial chemist prepares a 0.025 mol/L solution of hydrazoic acid, HN3(aq), a weak…

Q: (i) Define pH in words. The strong acid HClaq has a pH value of 1, use the following equation for a…

A: pH of a solution is the measurement of concentration of hydrogen ion in solution. pH stands for…

Q: The pH scale was designed to make it convenient to express hydrogen ion concentrations that are…

A: The pH of a solution determines the acidity or basicity nature of a solution. It is determined by…

Q: pH

Q: Write the acid ionization reaction for H2S04-

A: H2SO4 (sulfuric acid) is a diprotic acid which means it has two ionizable or replaceable protons.

Q: The acid dissociation constant K of acetic acid (HCH2CO2) is 1.8 × 105. Calculate the pH of a 2.7M…

A: The problem is asking us to calculate the pH of a 2.7M solution of acetic acid. The acid…

Q: 134 grams of potassium sorbate KCH3 (CH)4CO2 is fully dissolved in 100.00 mL of water, which is…

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

Q: -8 The base protonation constant K, of lidocaine (CH, NONH) is 1.15 × 10 °. 14 Calculate the pH of a…

Q: For the following acid-base reaction, (1) predict the products, showing both reactants and products…

Q: In a solution of 0.015 mol L HBr(aq) at 25 °C (a) What are the concentrations of the hydronium,…

A: Here we are required to find the pH of HBr

Q: Calculate pH of 2.5 x 10-3 M HCl(aq). HCl(aq) is strong base.

A: Give data The molar concentration of acid (HCl(aq)) = 2.5 x 10-3 M HCl(aq) is strong acid. pH of a…

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: Formic acid, HCOOH, ionizes in water according to the following equation. The equilibrium constant…

A: :- This question is answered by using the simple concept of ionisation of weak acid and then using…

Q: H^OH Determine the pH of the following 4 Carboxylic acids listed below using the provided pH…

A: HCOOH -----> H+ + HCOO- Let initial molarity of HCOOH = 1 M HCOOH…

Q: What is the pH of each of the following solutions? (Note that it may be necessary to use the…

Q: A monoprotic weak acid,HA, dissociates in water according to the reaction HA(aq)+H2O equilibrium…

Q: Determine the concentration of a NH Cl aqueous solution that has a pH = 5.975. The base ionization…

A: In this question, we have to find out the correct answer of given problem by the help of the…

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: The acid dissociation constant K of carbonic acid (H,CO,) is 4.5 x 10. Calculate the pH of a 2.0M…

A: ★ Answer : pH of 2.0 M carbonic acid solution is 3.0 ★ Solution : H2CO3 is a weak acid that…

Q: The concentration of hydronium ion in a sample is 3.5 x 10-7 mol/L. What is the pH of the above…

Q: What is the pH and the pOH of a 0.0125 M KOH solution at 100.0 °C? The value for Kw for water is…

A: Concentration of KOH solution as 0.0125 M at 100 °C

Q: The acid dissociation constant K, of acetic acid (HCH, CO,) is 1.8× 10¯³. a Calculate the pH of a…

A: Given Ka = 1.8*10-5 [Acid] = 0.47 M To find pH the formula used pH = pKa + log[Conjugate…

Q: OOO0 Solution) solution c mo mo mo ma

A: pH is the negative logarithm of the concentration of H+ ions. The scale of the pH is…

Q: Determine the pH of 0.080 M NH4Cl (pKa = 9.3). Give your answer to two decimal places.

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

Q: Calculate the pH and pOH of the following solutions (see Appendix 11 of your textbook for pKa…

A: "Since you have asked multiple questions and not mentioned the question number to be solved, we will…

Q: Answer the following questions. Write the expression for the equilibrium constant for the reaction…

A: NaCl is soluble and formation of ions and hence the concentration of ions to a high level . Kc =…

Q: The acid dissociation constant K, of carbonic acid (H,CO,) is 4.5 x 10 '. a Calculate the pH of a…

A: Given Ka for H2CO3 = 4.5 × 10-7 initial Concentration = 0.41 M

Q: What would be the pH of a solution that produces H3O+ ions at a concentration of 3.7 x 10-4 M? Write…

A: Concentration of hydronium ion , [H3O+] = 3.7×10-4 M To determine: pH of solution

Q: A solution is prepared at 25 °C that is initially 0.35M in nitrous acid (HNO2), a weak acid with K =…

A: Given: [HNO2]=0.35M;[NO2−]=1.2M;Ka=4.5x10−4Step 1: Write the dissociation of the weak…

Q: pH of a 0.223 M solution of sodium hydrogen chromate (K, 3.0 X 107)

A: Given data are as follows

Q: There is very little change to the pH of the solution. If anything the pH of the solution

A: If we add ammonium chloride in an ammonia solution. Then it acts as a basic buffer. Buffer is the…

Q: The acid dissociation constant K, of boric acid (H,BO,) is 5.8 x 10. Calculate the pH of a 3.2M…

A: PH of weak acid can be calculated by using the relation. PH = 1/2 [ PKa - logC].

Q: The base protonation constant K, of allantoin (C,H,N,O,NH,) is 9.12 x 10 °. Calculate the pH of a…

A: Given Initial Concentration = 0.47 M Kb = 9.12 × 10-6

Q: For the following reaction identify the acid, base, conjugate acid and conjugate base. iOH OH + ||…

A: Organic reactions can be defined as the reactions in which organic reactants react with each other…

Q: The base protonation constant X of ammonia (NH Calculate the pH of a 0.16 M solution of ammonia at…

Q: A solution of sodium cyanide, NaCN, has a pH of 11.40. How many grams of NaCN are in 245 mL of a…

A: Molarity is defined as moles of solute present per liter of solution.

Question

The acid dissociation constant \( K_a \) of carbonic acid \((\text{H}_2\text{CO}_3)\) is \(4.5 \times 10^{-7}\).

Calculate the pH of a \(1.6 \, \text{M}\) solution of carbonic acid. Round your answer to 1 decimal place.

**Input Field:**
pH = [ ]

**Buttons:**
- Clear (X)
- Undo (⟲)
- Help (?)

Expert Solution

This question has been solved!

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

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 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

10 The acid dissociation constant K, of boric acid (H,BO,) is 5.8 x 10 Calculate the pH of a 2.5M solution of boric acid. Round your answer to 1 decimal place. - 0 pH = || ?
Determine the pH of a solution that is 0.30 M CH3COOH and 0.50 M CH3COONa. Be sure your answer has the correct number of significant figures. Note: Reference the K of acids at 25 °C table for additional information. pH = x10 ×
What is the pH of a 0.24 M solution of oxalic acid, H2C204? The Ka1,2 values of oxalic acid are 5.6 x 102 and 5.4 x 10, respectively. pH = Use correct number of significant digits;
Determine the pH of a 1.2 M solution of ammonia, NH3, with K = 1.8 x 10.
Determine the pH of each of the following solutions (Ka and Kb values can be found in the appendices of your textbook or online): (a) 0.045 M hypochlorous acid; (b) 0.0068 M phenol; (c) 0.080 M hydroxylamine.
A chemist dissolves 866. mg of pure perchloric acid in enough water to make up 50. mL of solution. Calculate the pH of the solution. Be sure your answer has the correct number of significant digits. x10 ?
The value of K₂ for nitrous acid is 4.50×10-4. What is the value of K₁, for its conjugate base, NO₂? ||
Q3. This question is about the pH of several solutions. Give all values of pH to 2 decimal places. (a) (i) Write an expression for pH. (b) (ii) Calculate the pH of the solution formed when 10.0 cm³ of 0.154 mol dm-³ hydrochloric acid are added to 990 cm³ of water. The acid dissociation constant, Ka, for the weak acid HX has the value 4.83 x 10-5 mol dm-³ at 25 °C. A solution of HX has a pH of 2.48 Calculate the concentration of HX in the solution. Page 4 of 14
The base protonation constant K, of allantoin (C,H¸N,O,NH,) is 9.12 x 10 °. 4 3 Calculate the pH of a 0.46 M solution of allantoin at 25 °C. Round your answer to 1 decimal place. pH = || %D
Complete and balance each of the following equations for acid-base reactions. Express your answer as a chemical equation. Identify all of the phases in your answer. H2SO4(aq)+KOH(aq)→H2SO4(aq)+KOH(aq)→
What is the pH of a 0.10 M N(CH3)3(aq)? The base ionization constant of trimethylamine is Kb= 6.5×10–5. Enter your answer with correct units and significant figures.
Many common weak bases are derivatives of NH3, where one or more of the hydrogen atoms have been replaced by another substituent. Such reactions can be generically symbolized as NX3(aq) + H₂O(1) HNX3+ (aq) + OH- (aq) where NX3 is the base and HNX3 is the conjugate acid. The equilibrium-constant expression for this reaction is Kb = [HNX,'][OH ] [NX3] where K is the base ionization constant. The extent of ionization, and thus the strength of the base, increases as the value of K₁, increases. K and K are related through the equation K₂ x Kb = Kw As the strength of an acid increases, its K₂ value increase and the strength of the conjugate base decreases (smaller K₁, value). If Kb for NX3 is 2.0x10-6, what is the percent ionization of a 0.325 M aqueous solution of NX3? Express your answer numerically to three significant figures. ► View Available Hint(s) percent ionization = 27 Submit Previous Answers Request Answer * Incorrect; Try Again; 4 attempts remaining Part C ΠΙΑΣΦ If K₁, for NX3 is…