**Question:**Propionic acid, CH₃CH₂COOH, has a \( K_a = 1.34 \times 10^{-5} \). If 10.00 mL of 0.080 M propionic acid is mixed with 10.00 mL of 0.060 M KOH, what is the pH of the resulting solution?**Options:**- 4.40- 3.29- 3.44- 5.35- 4.87**Explanation:**The problem requires calculating the pH of a solution formed by mixing propionic acid with potassium hydroxide (KOH), a strong base. You will need to use the given \( K_a \) value for propionic acid and apply the concepts of acid-base reactions and buffer solutions. The options suggest possible pH values for the solution.

Answered: Image /qna-images/answer/5d6d79e8-8fd6-4886-8763-d76c722835cf.jpg

Propionic acid, CH3CH2COOH, has a Ka = 1.34 x 105. If 10.00 mL of 0.080 M propionic acid is mixed with 10.00 mL of 0.060 M KOH, what is the pH of the resulting solution? O 4.40 O 3.29 O 3.44 O 5.35 O 4.87

Propionic acid, CH3CH2COOH, has a Ka = 1.34 x 105. If 10.00 mL of 0.080 M propionic acid is mixed with 10.00 mL of 0.060 M KOH, what is the pH of the resulting solution? O 4.40 O 3.29 O 3.44 O 5.35 O 4.87

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: Phenylacetic acid (C6H5CH2COOH, simplified here as HPAc) builds up in the blood of persons with…

A: Answer: Given data: pH=2.62α=0.02C=0.12M

Q: Determine the pH of a solution that is prepared by dissolving 8 g of Ba(OH)2 in 3.8 L water at 25°C.…

A: pH is given by: pH = 14 - pOH = 14 - (-log[OH-]) = 14 + log [OH-]…

Q: Carbonic acid, H,CO, is a diprotic acid with Ka1 = 4.3 × 107 and Ka2 = 5.6 × 1011. What is the pH of…

A: H2CO3 ⇌HCO3− + H+......... ka1= 4.3x10-7 HCO3− ⇌CO3-2 + H+.......... Ka2=5.6x10-11ka1…

Q: A solution is prepared by dissolving 4.50 g of solid NaOH in 1.00 L o 0.100 M HNO₂(aq) (Ka =…

A: The pH of the solution can be calculated as follows

Q: Ka for HOCl is 3.2 × 10-8. How much chlorine (g) must be dissolved in 2.0 liter of water so that…

A: Given data are as follows Chemical reaction Cl2(g) + H2O(l) ⇌ H+(aq) + Cl–(aq) + HOCl(aq) Ka for…

Q: Which of the following solutions will have the lowest pH value? Group of answer choices 0.10 M HNO3…

Q: What is the pH of a 0.370 M solution of Ca(NO₂)₂ (Ka of HNO₂ is 4.5 × 10⁻⁴)?

A: Given : Concentration of Ca(NO2)2 = 0.370 M And Ka of HNO2 = 4.5 X 10-4 Since Ca(NO2)2 is a…

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

A: Given information: Ka for HOCl = 3.2 × 10-8 Volume of water = 3 litres. PH = 2.51 Given equation:…

Q: In a solution of equal concentrations of barbituric acid (C4 H 4 N 2 O 3 ) and sodium barbiturate (C…

A: A mixture of weak acid and its conjugate ion with strong base forms an acidic buffer solution. A…

Q: What is the pH of a 0.24 M solution of sodium propionate, NaC3H5O2, (base) at 25°C? (For propionic…

Q: Milk of magnesia is a suspension of magnesium hydroxide in water. Although Mg(OH)2 is relatively…

A: pH of milk of magnesia = 10.08 volume of milk of magnesia = 3.6 tablespoons

Q: Acetic acid (pKa = 4.75) is contained in vinegar. Calculate the pH of the solution prepared by…

A: First to calculate molarity Then to calculate pH using formula.

Q: Assume the following substances form solutions at the same concentration, whicch one would provide…

A: According to Arrhenius concept, an acid is a substance i.e. when dissolved in water gives H+ ions.…

Q: What is the pH of a 0.320 M solution of Ca(NO₂)₂ (Ka of HNO₂ is 4.5 × 10⁻⁴)?

Q: HCIO 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: Kw = Ka x Kb Kw = 1x10-14 given that Ka = 4x10-8 find Kb = (1x10-14) / (4x10-8) = 2.5x10-7 Initial…

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: The pH of dissolving 1.48 g of propanoic acid (CH3CH2COOH, Ka 1.3X105) in 200 mL H20 is 4.82 O 3.71…

Q: Substance 0.1 M HNO3 0.1 M KCI 0.1 M Na₂CO3 0.1 M HC,H,O, 0.1 M NH OH Tap water Apple Juice 0.1 M…

Q: The pH of a 0.45 M solution of a weak acid, HA, is 2.13. What is the value of Ka for the weak acid?

A: Given data,pH=2.13Molarity of HA=0.45

Q: What is the pH of a solution that contains 6.13 x 10–4 M OH–?

A: pH measures the acidity of the solution whereas pOH measures the basicity of the solution -

Q: Rainwater that falls close to a power plant has H3O+ ion concentration of 6.25x10-4. What is the…

A: Formula of pH pH = -log[H+] or pH = -log [H3O+]

Q: ated with a 0.0985 M NAOH solution, v of the solution when 25.00 mL of NaO

A: We will calculate pH

Q: NH3 is a weak base (Kü = 1.8 x 10-5) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

A: Kb value of ammonia = Concentration of NH4Cl= 0.046 MDetermine the pH of solution.

Q: The pH of the 0.50 M solution of HA is 1.92. What is [HA]?

A: Answer:pH is equal to negative of logarithm of hydrogen ion concentration in solution, so,

Q: A solution of acids is made by mixing 0.19 M HNO3 and 0.45 M CH3COOH (Ka (CH3COOH) = 1.8 x 10-5).…

A: To calculate the pH of the solution, we need to consider the acid dissociation reactions of both…

Q: HCIO is a weak acid (Ka 4.0 x 10-8) and so the salt NaCIO acts as a weak base. What is the pH of a…

A: Given data; Ka=4×10-8Also, Kw=Ka×KbAnd,Kw=1×10-14 Consider the dissociation of given weak acid as;…

Q: What is the pH of a 0.17 M weak acid solution? The KA of the weak acid is 2.1 x 10-5.

A: Given :- Initial concentration of weak acid = 0.17 M Ka for acid = 2.1 × 10-5 To be calculated :-…

Q: A titration of 0.100 M NaOH is titrated into 25.0ml of a 0.100 M HCHO2 solution (Ka = 1.80 x 10 4).…

Q: What is the pH of a 0.820 M solution of Ca(NO₂)₂ (Ka of HNO₂ is 4.5 × 10⁻⁴)?

A: The pH of the solution is equal to the negative logarithm of hydronium ion while pOH of the solution…

Q: A 0.60 M solution of a weak acid, HA, has a pH of 3.41. What is the percentage ionization of the…

A: ★ Answer : percentage of ionization of the acid is 0.064%

Q: Morphine, C 17H 19NO 3, is often used to control severe post-operative pain. What is the pH of the…

A: Which one of the following is correct answer

Q: If 34.6 mL of a 0.68 M NaOH solution is added to a 51.9 mL sample of a 0.68 M weak acid, HA , what…

A: 34.6 mL of a 0.68 M NaOH solution is added to 51.9 mL sample of a 0.68 M weak acid, HA (ka = 1.8 x…

Q: It is believed that a bath in Epsom Salts can relieve various types of pain. In preparation for…

Q: The concentration of H* (or H3O*) from part A should be 1.02x×10-2 mol L-1. What is the pH of the…

Q: 546.0 mL of a 0.13 M solution of ammonia is mixed with 546.0 mL of a 0.13 M solution of HBr. What is…

A: The question is based on the titrations. we are titrating a strong acid hydrobromic acid with a…

Q: What is the pH of 1.000 L of a solution of 100.0 g of glutamic acid (C5H9NO4, a diprotic acid; K1 =…

Q: How to calculate the ph? What would be the result if the acid was a di or tripotic? How do the…

A: All of your concerns are discussed; please go through each step.Explanation:Step 1: Let's learn…

Q: Milk of magnesia is a suspension of magnesium hydroxide in water. Although Mg(OH)2 is relatively…

A: given, pH of solution = 10.08

Q: A solution is made by dissolving 15.1 g of CH₃NH₃NO₃ in 500.0 mL of water. Using Ka(CH₃NH₃⁺) = 2.3 ×…

Q: What is the pH of the following solution? 30.0 mL of 0.41 M HOCI (Ka = 2.8 x 10-8) is added to 30.00…

A: We have to calculate the pH of solution

Q: You have 50.0 mL 0.10 M NazPO4 to which you add 50.0 mL 0.19 M NaH PO4. What is the pH of this…

A: We can calculate the pH of the solution using the formula, Calculate the total volume of the…

Q: Which conformation of cyclohexane has the greater steric strain?

Q: Calculate the pH of a solution that is a mixture of 0.030M HNO3, 0.55M CH3COOH, and 0.015M HI. Ka…

A: Given data : HNO3 = 0.030 M HI = 0.015 M CH3COOH = 0.55 M

Q: what is the pH of a solution containing 7.1 g of acetic acid (HC2H3O2) dissolved in 240 mL of water?…

A: Acetic acid i.e CH3COOH is a weak monoprotic acid. Hence it will dissociate partially in the…

Question

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 with 2 images

SEE SOLUTION Check out a sample Q&A here

Similar questions

a) What is the pH of 0.001 M HCl (strong acid)? b) What is the pH of 0.010 M NaOH (strong base)? c) Acetic acid is a weak acid. Calculate the pH of a 0.08 M aqueous solution given that the Ka for acetic acid = 1.8 x 10-5.
You are asked to find the pH of each solution described below. A 0.50 M solution of HBrO3 A 0.030 M solution of Ca(OH)2 A 0.50 M solution of NH4Br A solution that is 0.20 M in NH3 and 0.35 M in NH4NO3 after the addition of a small amount of NaOH A solution that is 0.40 M in HCOOH and 0.30 M in NaHCOO A 0.25 M solution of CH3NH2 Options： A.weak acid B.strong acid C.weak base D.strong base E.acid salt F.basic salt G.buff by it self H.buff after add strong base I.buff after add strong acid
A strong base, such as sodium hydroxide (NAOH), is added in a solution of 0.1 mol/L acetic acid (CH3COOH, pka = 4.7). The pH after the addition of the strong base is 10. What is the concentration of acetic acid (CH3COOH) in the solution in mol/L after the addition of the base? O 5 10-6 mol/L O 0.1 mol/L 10-10 mol/L O 0.009 mol/L
For the acid HA, the acid dissociation constant, Ka, is 1.1 x 105. After 48 mL of 0.9 M NaOH is added to 48 mL of a 1.8 M HA solution, what will the pH of the resulting solution be?
1.) HA is a weak acid. Its ionization constant, Ka, is 3.1 x 10-13. Calculate the pH of an aqueous solution with an initial NaA concentration of 0.061 M. 2.) We place 0.149 mol of a weak acid, HA, in enough water to produce 1.00 L of solution. The final pH of the solution is 1.11 . Calculate the ionization contant, Ka, of HA. 3.)We place 0.527 mol of a weak acid, HA, and 12.0 g of NaOH in enough water to produce 1.00 L of solution. The final pH of this solution is 4.35 . Calculate the ionization constant, Ka, of HA.
a) What is the pH and pOH of 0.001 M NaOH solution, which is the strong base? b) The Ka value of CH3COOH is 1.8x10-5. What is the molar concentration of H ions in a 5x 10-2 M acid solution?
5 mg of HNO3, which is a strong acid, is added to 750 ml of water. What is the final pH of the solution?
The pH of a 0.224 M solution of a weak acid, НВ, is 2.63. What is Ka for the weak 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 x10 -10. A solution of phenol is prepared by dissolving 14.5 g of phenol in enough water to make 892 mL of solution. For this solution, calculate pH
Calculate the pH of the following solutions. Ka for HClO is 2.5*10-9 a)A solution made by dissolving 4.50 g hypochlorous acid (HClO) into 1.50 L of solution. b)A solution made by dissolving 7.40 g of potassium hypochlorite (KClO) into 1.50 L of solution. c)A buffer is prepared by adding 4.50 grams of hypochlorous acid (HClO, Ka=2.5*10-9) and 7.40 grams of potassium hypochlorite (KClO) to a make a 1.50 L solution.
Instant cold packs are usually comprised of a small packet of solid, when upon dissolution in water, undergoes an endothermic reaction. One such compound used in everyday cold packs is ammonium nitrate, NH4NO3. Calculate the pH of a cold pack if the initial molarity of ammonium nitrate is 0.15 M. The K for ammonia, NH3, is 1.8x10-5.
When 4.73 g of the weak acid HC6H4CIO is dissolved in 800 mL of solution, the pH is 5.25. What is the Ką of HC6H4CIO? (Note: This acid is not listed in Table 2.) O 5.3 x 10-12 O 8.6 x 10-10 O 3.2 x 10-11 O 1.2 x 10-4 O 6.9 x 10-1o