Answered: A scientist is looking for the K, of an…

A scientist is looking for the K, of an unknown acid, HA. When 5 moles of HA and 10 moles of NaA are added to 1000 mL of water, the pH is 8.12 . What is the K, of the unknown acid?

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: A weak acid, HA, has a p?apKa of 4.5424.542. If a solution of this acid has a pH of 4.4944.494, what…

Q: Giycolic acid is often used in skin care products. A saturated solution of its calcium salt has a…

Q: Lemons get their sour flavor from citric acid (Ka = 7.4 x 10-4) a fresh squeezed lemon can have a…

Q: HF is a weak acid and NH3 is a weak base. Which of the following shows the correct order of…

A: Sodium chloride is formed from the reaction of a strong acid and a strong base. In the formation of…

Q: You have a bottle that is 2.5 L and 12 Molar HCI. What is the pH of the acid? How many moles of HCI?

A: Answer:- This question is answered by using the simple concept of calulation of pH of strong acid…

Q: Aspirin, a drug that is used to relieve minor aches and pain, is a weak monoprotic acid. What is the…

A: we know that pH = -log [H+] so -log [H+] = 3.12 [H+] = 0.000758

Q: A solution is prepared by dissolving 0.89 mol of a weak base in 1.00 L of water. The resulting pH at…

A: Dissociation of a weak base and pOH calculation

Q: Question 1 Calculate the pH of the resulting solution when 22.0 mL of 0.12 M KOH are added to 28.0…

A: In this question we have to tell the PH of the resulting solution.

Q: Hydrofluoric acid (HF) has a Ka value of 7.2 x 10-4. What is the pH to 2 decimal places when 6.875…

A: When weak acid HF reacts with KOH to form a buffer solution . The pH of buffer solution can be…

Q: Explain why the pH does not change significantly when a small amount of an acid or a base is added…

A: The solution of a weak acid or base with its conjugate base or acid respectively is known as a…

Q: What is the pH of a solution that contains 0.10 M cyanic acid and 0.20 M sodium cyanate?

Q: A 0.22 M solution of a weak monoprotic acid, HA, has a pH of 3.28. Calculate Ka for the acid. 1.5 ×…

A: Given, pH = 3.28 Concentration of weak monoprotic acid= 0.22M

Q: A solution of sodium hypochlorite is made in 2.0 L of water. The pH is determined to be 10.50.…

Q: A chemist makes a new solution: 1.0 L of a solution that is both that is both 0.6 M NH3 and 0.8 M…

A: Henderson Hasselbach equation is used to calculate the pH of a buffer system . pH=pKa +…

Q: In a 1.18 M aqueous solution of a monoprotic acid, 3.81% of the acid is ionized. What is the value…

A: Acid dissociation constant ka is given by equilibrium concentration of product divided by…

Q: t is the pH of a 0. M solutI 350 M solution of NaOH is added? The K, of HA is 4.3 x 10-4.

A: We have to tell which option is correct from given choices of options by telling what is the pH of…

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

A: The ionization of NH4Cl as follows,

Q: 1. K, for vitamin C (also known as ascorbic acid, CH,O.) is 8.0 x 10. If 13.5 g of vitamin C is…

Q: What is the value of Ka of this acid? What is the percent ionization of this acid?

Q: Acrylic acid, whose formula is HC; HOz or HO, CCH-CH2, is used in the manufacture of plastics. A…

Q: 6.5 g of sodium acetate was dissolved in 100 mL of water to give a final volume of 106 mL. If the Ka…

A: Sodium acetate dissociates in water into sodium and acetate ions. Sodium ions react very little with…

Q: Enough of a monoprotic weak acid is dissolved in water to produce a 0.0176 M solution. The pH of the…

A: given values are - initial concentration of monoprotic acid = 0.0176 M pH = 2.47 Ka = ?

Q: You need to achieve a pH or 6.8-7.2. You have 113 mL excess 5.13 M HCI. How many grams of solid NaOH…

A: Neutralization reaction occurs when an acid and base reacts to produce salt and water. It involves…

Q: en 13.75 mL of a 1.074 M solution of KOH has been added to a 27.5 mL f hydrofluoric acid with a…

A: We will calculate pH

Q: If a 0.8M solution of weak acid, HA, has a pH = 2.8, calculate the Ka of the acid. Your answer…

A: HA ⇌ H+ + A- At initial c 0 0at final c1-α…

Q: If you are titrating a 20.0 mL of a 0.100 M solution of HCl with 0.100 M NaOH, what is the pH of…

Q: What is the pH of a solution resulting from 5.00 mL of 0.075 M NaOH being added to 45.00 mL. of pure…

A: To calculate the pH of the resulting solution, we need to determine the concentration of hydroxide…

Q: If you were to make a 1L sodium hydroxide solution from 1.5 g of NaOH, what would be the pH of a…

A: pH of a solution is the negative logarithm of hydrogen ion concentration. pH = -log[H+] pOH = -log…

Q: A student has a sample of 0.50 M lactic acid (HC 3H5O 3). She adds 10 mL of this solution to 40 mL…

A: The objective of the question is to write a chemical reaction for the dissociation of lactic acid in…

Q: solution of HCN was prepared in 2.5 L of water. The pH of this solution at 25°C was determined to…

A: HCN is a weak acid, it does not dissociate completely. (

Q: A chemist makes a 1.0 L of a solution that is both 0.6 M NH, and 0.8 M NH,CI. pK, of NH3 = 4.75.…

A: Given :- Concentration of NH3 solution = 0.6 M Concentration of NH4Cl = 0.8 M Volume = 1 L pKb…

Q: A chemist dissolves 206, mg of pure perchiloric acid in enough water to make up 240. ml of solution.…

A: pH of a solution measures the acidity of the solution. Now, perchloric acid is a strong acid hence…

Q: Consider 0.10 M solutions of the following compounds: Sr(OH)2, Ca(OCl)2, FeCl3, Ca(C3H5O3)2, and…

A: Sr(OH)2 is a strong base and will have the highest pH. Ca(C3H5O3)2 is a weak base and will have a…

Q: alculate the pH of each of the following buffered solutions: 0.25 M acetic acid CH3COOH (Ka = 1.8 x…

A: Given,Concentration of Acetic Acid = [CH3COOH] = 0.25 MConcentration Sodium acetate = [CH3COONa] =…

Q: If you mix 23.6 g of KOH in 16.5 liters of water, what is the pH?

A: pH is defined as the negative logarithm to the base 10 of H+ ion Concentration expressed in mol/L.…

Q: What is the pH of a solution that is 0.34 M KOCN and 0.14 M HOCN (cyanic acid)?

Q: if a student add a solution of 0.10 M NaOH to 20.0 mL of 0.10 M HF (ka=3.50×10-4 ) until it reaches…

A: Given that Molarity of HF = 0.10 M Volume of HF = 20.0 mL Ka of HF= 3.5 x 10-4 Concentration…

Q: What is the Ka of a weak acid whose 0.10 M solution produces a pH of 2.38?

Q: A 1.0 M solution of a weak acid, HA has a pH of 2.64. What is the value of Ka for this acid?

A: The acidic strength of all known acids is dependent on their dissociation constants. This constant…

Q: Chemistry

Q: for HA. A 0.15 M solution of the weak acid HA has a pH of 3.75. Find the value of K

Q: pH of a 0.30 M solution of a weak base B is 9.02. What is the K, of the base? Be sure your answer…

Q: M H,SO4. The resulting solution has a pH

A: Applying molarity equation and pH formula MV= M1V1- M2V2 PH = -log (H+)

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

A scientist is looking for the K, of an unknown acid, HA. When 5 moles of HA and 10 moles of NaA are
added to 1000 mL of water, the pH is 8.12 . What is the K, of the unknown acid?

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 with 2 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

A 1.57 M solution of a weak acid HA is found to have a pH of 2.05. Determine the pH of a 2.00 M solution of the sodium salt, NaA
Hydrofluoric acid (HF) has a Ka value of 7.2 x 10-4. What is the pH to 2 decimal places when 17.20 mL of a 1.074 M solution of KOH has been added to a 27.5 mL solution of hydrofluoric acid with a concentration of 0.537 M.
A 0.175 M weak base has a pH of 8.86. What is the K value of this base? K
Calculate the pH of the glacial acetic acid and the solution you prepared in step 1. Step 1: Glacial acetic acid, the most concentrated CH3COOH you can buy, has a concentration of 17.54 M. Calculate the concentration of CH3COOH is a solution that is prepared by combining 15.0 mL of glacial acetic acid with enough water to make 250-mL of solution. (Please be very detailed when answering the question)
Consider the following reaction at equilibrium. CH,COOH(aq) = CHyco0 (aq) + H*(aq) When NaCH3CO0 is added to the solution will the value of the equilibrium constant, K, and the pH of the solution increase, decrease, or remain the same? Select one: O A. K, decreases and pH increases O B. Ka remains the same and pH decreases O C. Ka decreases and pH remains the same O D. K, remains the same and pH increases O E. K, increases and pH decreases
-A 2.5 M solution of a weak acid, HA, is 1.8% ionized in water. What is the K, value for this weak acid?
The pH of a 0.20 M solution of some weak acid HX is 4.22. What is the Ka value of this acid?
The hydronium ion concentration in a sample of rainwater from a remote location is found to be 1.7 x 10−6 M at 25 °C. a) What is the concentration of hydroxide ions in the rainwater? b) What is the pH of the rainwater sample? c) Acid rain can have hydronium ion concentrations as high as 6.3 x 10-5 M. What is the pH of acid rain?
1.) In a 0.100M aqueous solution of a weak acid, the acid is 3.7% dissociated. What is the Ka for this acid? 2.) What is the pH of a 0.010M solution of pyridine, C2H5N, a weak base? It's Kb is 1.5x10-9. 3.) Calculate the pH and percent ionization of a 15.0 M solution of a weak base. (pKa=9.26) SHOW ALL WORK!!
Calculate the pH of a solution that contains 0.00415 M HI and 0.400 M benzoic acid. (Ka for benzoic acid is 6.5×10−5)
A 0.255 M solution of a weak acid, HA, has a pH of 3.24. Calculate the Ka for the acid.
Hypobromous acid, HBrO, can be produced commercially as a disinfectant. A solution is made by dissolving 3.73 kg of pure HBrO in distilled water to make 10.0 L of solution. A pH pribe determines that the pH of the aqueous solution is 3.98. What is the value of Ka for HBrO?