Calculate the equilibrium molar concentration of a weak acid HA (154.5 g/mol) if 200 mg of that acid is dissolved in water to prepare a 10 mL solution. Given that the HA is 45 % ionized. 1. O0.712 M 2. O0.0712 M 3. O0.058 M 4. O0.129 M

Calculate the equilibrium molar concentration of a weak acid HA (154.5 g/mol) if 200 mg of that acid is dissolved in water to prepare a 10 mL solution. Given that the HA is 45 % ionized. 1. O0.712 M 2. O0.0712 M 3. O0.058 M 4. O0.129 M

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: What is the difference between a strong acid and a weak acid? Strong acids completely dissociate in…

A: Strong acids are substances that completely dissociate into ions when dissolved in water, breaking…

Q: Identify whether each species functions as a Brønsted-Lowry acid or a Brønsted-Lowry base in this…

Q: Consider the following data on some weak acids and weak bases: name formula HNO₂ 4.5 x 10 acetic…

A: The question is based on the concept of salt hydrolysis.We need to arrange the given salts in…

Q: The pH of an aqueous solution at 25°C was found to be 5.10. The pOH of this solution is . The…

Q: Calculate the pH of each of the following solutions. Ka(НС2 Н3О2) %3D 1.8 х 10 5 Ка(НCN) — 6.2 х 10…

A: #(a): KC2H3O2(aq) is a conjugate base of HC2H3O2(aq). Hence it will undergo hydrolysis to form…

Q: Identify whether each species functions as a Brønsted-Lowry acid or a Brønsted-Lowry base in this…

A: Bronsted-Lowry Acid - Base :- An acid is a substance which gives H+ and form i conjugate…

Q: Identify whether each species functions as a Brønsted-Lowry acid or a Brønsted-Lowry base in this…

Q: What is the Ka of cyanuric acid if a 0.030 M cyanuric acid aqueous solution has a pH of 4.15? O…

Q: Determine the pH of the following: a single solution prepared to final concentrations of 0.01469 M…

A: pH is the negative logarithm of hydrogen ion concentration. When an acid is mixed with a base, both…

Q: What is the pH of a barium hydroxide solution obtained by dissolving 0.27 grams of barium hydroxide…

Q: Which solution has the highest pH? O 0.065 M HIO (Ka-2.3x10-11) O 3.5x10-4M HBrO (Ka-2.5x10-9) O…

Q: A solution is 0.00476 M HCl. What is the concentration of HCl molecules and H3O+ ions molecules in…

A: Since HCl is a strong acid, it dissociates completely in the solution. The concentration of HCl…

Q: If the pOH of an aqueous NaOH solution is 11.55, what is the [H3O+] for this solution? 6.8 x 10-8 M…

A: Given: The pOH of an aqueous NaOH (sodium hydroxide) solution is 11.55. [H3O+] is the concentration…

Q: The solution that was prepared has a pH of 5.61. How many hydroxide ions are pr esent in the…

Q: Each value represents a different aqueous solution at 25 °C. Classify each solution as acidic,…

A: Hydrogen ion concentration is an important parameter of an aqueous solution. The concentration of…

Q: I. Calculate pH from the following hydrogen ion concentration (M). Identify each as an acidic pH or…

A: Since you have asked multiparts questions, we will solve the first three sub parts questions for…

Q: The pH of an aqueous solution at 25°C was found to be 3.10. The pOH of this solution is _____.…

A: pH = -log [H+] [H+] = 10-pH pOH = -log [OH-] [OH-] = 10-pOH pH + pOH = 14

Q: A solution is made by dissolving 48.9 g of Ba(NO2)2 in 500.0 mL of water. As NO2¯ is a base, write…

A: Answer:- This question is answered by using the simple concept of hydrolysis of salt of weak acid…

Q: The hydronium ion concentration in an aqueous solution at 25°C is 4.2×10² M. The hydroxide ion…

A: Given that: [H3O+] = 4.2×10-2 M

Q: Weak Acid HCN HNO HIO HBrO CHCOOH K₂ 4.9 x 1010 4.5 x 10 2.3 x 10¹1 2.5 x 10 6.3 x 10* Which of the…

A: 4 saltCsIONaFLiClO3KNO2Solutions would be expected to have a pH of 7.00 = To be determined

Q: What is the pOH of an aqueous solution of 0.216 M hydroiodic acid? pOH = ___________

Q: Identify whether each species functions as a Brønsted-Lowry acid or a Brønsted-Lowry base in this…

A: Since, From the definition, Brønsted-Lowry acid are proton donar and Brønsted-Lowry base are proton…

Q: 0.117 M solution of a weak base has a pH of 11.77. What is the value of K, for the weak base? Kb =

A: In this question, we will determine the Kb value of weak base. Given that, Concentration of weak…

Q: Ka formula hypochlorous acid HClO 3.0 x 10 HNO₂ 4.5×10 name acid nitrous acid solution. 0.1 M KNO₂…

Q: A solution is prepared by adding 49.7 mL concentrated hydrochloric acid and 19.1 mL concentrated…

A: Given: The volume of concentrated hydrochloric acid (HCl) is 49.7 mL The volume of concentrated…

Q: Which of the following is identified as a weak base? LİOH - Ва(ОН)2 NH4OH NaOH

A: Weak base from above four option is

Q: The ion-product constant for water, Kw, is expressed in the following equation: Kw = [H+] x [OH] =…

A: Given: [OH-] = 0.0300 mol/L

Q: A solution is prepared by dissolving 0.0200 mole of HCl and 0.0100 mole of KOH in enough water to…

A: The first part of the question is asking for the standard Gibbs free energy change (ΔG°) for the…

Q: A certain weak base has a ?bKb of 8.80×10−7.8.80×10−7. What concentration of this base will produce…

A: 0.057 M

Q: NH3 is a weak base (?b=1.8×10−5) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

A: Calculating for pH given the value Kb :- In solving this problem we need the right dissociation…

Q: In a solution of hydrochloric acid in water, the concentration of hydrogen ions is 10-2M. What is…

Q: culate the hydronium ion concentration (in M) of a blood sample with a pOH of 7.8.

Q: The pH of 0.10 M solution of an acid is 6. What is the percentage ionization of the acid? 6.0 %…

A: Given, pH = 6. Concentration of solution = 0.10M. The dissociation of acid can be given as follows:

Q: A solution is made with 3.825 g NH,CI, dissolved in enough water to make 625 mL of solution. If the…

A: First, we calculate the concentration of the solution. After that, we calculate the [OH-] with the…

Q: ľ The pH found to The hydr The hyd.

Q: Identify whether each species functions as a Brønsted-Lowry acid or a Brønsted-Lowry base in this…

A: The species that donate H+ are bronsted lowry acids while those that accept H+ are bronsted lowry…

Q: A 0.025 M solution of acetic acid (CH3COOH) is 4.2% ionized. What is the pH of this solution? O2.14…

A: The objective of the question is to determine the pH of the given solution.It is given that,The…

Q: Which aqueous solution has the highest pH? O 0.55 M Ba(OH)2 O 1.0 M HCN 0 1.4 М СН3СООН O 1.2 M…

A: PH depend acid, base and salt. Strong acid lower Ph and strong base high Ph

Q: The pH of a 0.100 M CH3NH2 solution is 11.80. What is the % ionization value? O 11.80% O 1.58% O…

Q: In a solution of acetic acid in water, the pH is 5.0. Which expression identifies the concentration…

A: pH of a solution is the negative logarithm of hydrogen ion concentration. pH=-logH+…

Q: Which solution below has the highest concentration of hydroxide ions? pH = 8.2 pH = 5.6 pH = 3.7 pH…

Q: What is the percent ionization of a 0.15 M solution of weak acid that has a pH of 1.86?

Q: 4. The pH of a 0.030 M formic acid (HCOOH) solution is 2.63. If 0.030 M sodium formate (NaHCOO) is…

A: The solubility of sparingly soluble salt decreases when a solution having common ion is added to it.…

Q: Consider the following data on some weak acids and weak bases: name acetic acid hypochlorous acid…

A: The question is based on the concept of salt hydrolysis. we need to arrange the given salts in…

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

Calculate the equilibrium molar concentration of a weak acid HA (154.5 g/mol) if 200 mg of that acid is dissolved in water
to prepare a 10 mL solution. Given that the HA is 45% ionized.
1. 00.712 M
2. O0.0712 M
3. O0.058 M
4. O0.129 M

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 by step

Solved in 2 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

Each value represents a different aqueous solution at 25 °C. Classify each solution as acidic, basic, or neutral. Incorrect Acidic pH = 4.57 pOH = 4.97 pOH = 9.52 [H+] = = 9.8 x 10-5 Basic pH = 9.45 [H+] = 5.5 x 10-¹¹ [OH-] = 4.9 × 10-¹1 [OH-] = 5.4 x 10-² Answer Bank Neutral [H+] = 1.0 x 10-7 pOH = 7.00
Enough of a monoprotic acid is dissolved in water to produce a 0.0162 M solution. The pH of the resulting solution is 2.57. Calculate the K₁ for the acid. K₁ = M
Determine the pH of each two-component solution. a. 0.050 M KOH and 0.015 M Ba(OH)2 b. 0.265 M NH4NO3 and 0.102 M HCN c. 0.075 M RbOH and 0.100 M NaHCO3 d. 0.088 M HClO4 and 0.022 M KOH e. 0.115 M NaClO and 0.0500 M KI
What is the pH and percent ionization in a 0.145 M solution of sulfurous acid?
Determine the [OH] in a 0.15 M solution of sodium formate, a weak base whose K, is 5.6 x 104. O 7.5x106 M ○ 2.9x106 M O 5.2×10-3 M O 1.3×102 M
Each value represents a different aqueous solution at 25 °C. Classify each solution as acidic, basic, or neutral. Acidic Basic Neutral pH = 3.53 pH = = 12.01 %3D [H* : = 1.1 × 10–6 H+] = 5.2 x 10-10 РОН 3D = 2.59 [OH] = 9.4 x 10-9 РОН 3D 12.04 [H* = 1.0 × 10-7 [OH] = 7.5 x 10-6 РОН — 7.00
Consider the following data on some weak acids and weak bases: name acetic acid acid hydrocyanic acid solution 0.1 M NH4Br 0.1 M NaNO3 formula HCH,CO₂ HCN 0,1MKCN 0.1 M NaCH,CO₂ Ka 1.8 x 10-5 4.9 x 10-10 Use this data to rank the following solutions in order of increasing pH. In other words, select a 'I' next to the solution that will have the i the solution that will have the next lowest pH, and so on. X PH choose one choose one choose one v choose one S base name K₂ formula ethylamine C₂H₂NH₂ 6.4×104 NH, 1.8×10 5 ammonia
The pH of a nitric acid (HNO:) solution is 3.85 Determine the [H*] in the HNO3 solution. Calculate the number of moles of H* in 350.0 mL of the solution. Write the balanced chemical equation for the dissociation of HNO3. Hint: HNO3 is a strong acid. Calculate the number of moles of NO3 ions in 350.0 mL of the above solution. Consider the balanced chemical equation written in part (c).
At 25 °C, which aqueous solution has the lowest pH? O 0.17 M HNO2 O 0.15 M HNO3 O 0.20 M HCOOH O 0.20 M CH3CO2H
The pH of a 0.030 M formic acid (HCOOH) solution is 2.63. If 0.030 M sodium formate (NaHCOO) is added, which of the following statements will be true? A. the pH will decrease B. the equilibrium position shifts to the left C. the [H3O+] will increase D. the [HCOOH] will decrease
The pH of an aqueous solution at 25°C was found to be 12.00. The pOH of this solution is . The hydronium ion concentration is M. The hydroxide ion concentration is M.
The hydroxide ion concentration in an aqueous solution at 25°C is 2.2×102 M. The hydronium ion concentration is М. The pH of this solution is The pOH is