**Participation Question**1. What is the $[H_3O^+]$ of 0.10 M propanoic acid ($CH_3CH_2COOH$, can simplify to HPr) ($K_a = 1.3 \times 10^{-5}$)?2. Calculate the pH of a 0.050 M solution of ethylamine ($C_2H_5NH_2$, $K_b = 6.4 \times 10^{-4}$).

Answered: PARTICIPATION openstax What is the…

PARTICIPATION openstax What is the [H,O*) of 0.10 M propanoic acid (CH,CH,COOH, can simplify to HPr) (K, = 1.3x10-5)? Calculate the pH of a 0.050 M solution of ethylamine (C,H;NH2, Kb= 6.4 x104).

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: The pH of an aqueous solution of 0.170 M sodium acetate, NaCH3COO, is | (Assume that Ka (HCH3COO) =…

A: The question is based on the concept of the pH of the solution.It is defined as a negative logarithm…

Q: The pH of an aqueous solution of 0.415 M aniline (a weak base with the formula C,H&NH,) is

Q: 15) Which of the following is the weakest acid? SH OH NH, d) SH

A: From given compounds there is need to find weakest acid among all compounds.

Q: Part A Calculate the pH in 1.82 M CH,CO,H. Express your answer using two decimal places. pH= Part B…

A: Given, Concentration of CH3COOH, [CH3COOH] = 1.82 M To find- (A) The pH of acetic acid (B)…

Q: Which of the following 0.10 M acid solutions is expected to have a lower pH than 0.10 M CHBr₂COOH?…

Q: A chemist dissolves 417. mg of pure potassium hydroxide in enough water to make up 160. mL of…

A: Applying concept of molarity and PH and POH. POH= -log [OH-]

Q: The acid dissociation constant K, of alloxanic acid (HC,H,N,0,) is 2.24 x 1 Calculate the pH of a…

Q: Classify each solution as acidic, basic, or Neutral [H*] = 1.0 x 10-7 %3D pOH = 7.00 %3D

A: A) pH < 7 ( Acidic ) , pH > 7 ( basic ) and pH = 7 ( neutral ) B) All the Formula : pH + pOH…

Q: a) 25.0 ml of 0.80M KCI + 35.0 ml of 0.40M KOH b) 20.0 ml of .20M HCI + 30.0 ml of 0.10M NaOH c)…

Q: The ka of an unknown acid, HYO2, is determined to be 5 x 102 empirically. What is the pH of a 0.1 M…

A: Given that concentration of HYO2= 0.1 M Ka of HYO2 = 5 x 10−2 = 0.05

Q: 2-

A: Since pOH =14 + log[H+ ] => [H+] = concentration of H+ ions = 10pOH - 14 = 107.37 - 14 = 2.344 X…

Q: Part A) Calculate the pH and the concentration of C202-4 ions in 0.18 M H2C2O4 (Kal Ka2 = 6.4x10^-5)…

Q: A solution is prepared at 25 °C that is initially 0.35M in diethylamine ((C₂H3)₂NH), bromide…

A: pH + pOH = 14

Q: A solution is prepared at 25 °C that is initially 0.12 M in diethylamine ((C,H), NH), a weak base…

Q: A. Calculate the pH of 35.00 mL of acetic acid using the concentration assigned in Beyond Labz:…

A: We are given a problem based on ICE table, we have to complete the steps.

Q: Determine the pH of a solution that is 0.075 M (CH3),N and 0.10 M (CH3),NHCI. The value of Kb for…

A: Using Henderson hasselbalch equation:-

Q: Text Quest The pH values of two liquids are 3 and 6. Indicate which liquid is more acidic and how…

Q: 10. The pH of 0.25 M aqueous solution of a weak acid HA is observed to be 4.15. Determine the acid…

Q: The acid dissociation constant K, of carbonic acid (H,CO,) is 4.5 x 10. Calculate the pH of a 2.9 M…

Q: Which of the following statements is true? (Select all that apply.) In an acid solution, K₂ =…

A: Answer:Any specie that loses H+ ion in its solution is called as Bronsted-Lowry acid and the specie…

Q: None

A: 1. Write the Equilibrium Constant Expression (Ka) for HX dissociation:HX (aq) + H2O (l) <=>…

Q: A solution is prepared at 25 °C that is initially 0.29 M in trimethylamine ((CH,),N), a weak base…

Q: 4) Consider the polyprotic acid H₂C2O4 (Ka1 = 5.9 x 102 and Ka2 = 6.4 x 10-5). a. Write out the…

Q: Calculate the pH at 25 °C of a 0.52M solution of trimethylammonium chloride ((CH,) NHCI). Note that…

A: pKb for (CH3)3N = 4.19 pKa for (CH3)3NH+ = 14 - pKb = 14 - 4.19 = 9.81 Ka = 10–9.81=1.55 × 10–10 The…

Q: b. Calculate the pH of a 0.15 M pyridine solution. C;H;NH' (a9) OH (aq) C

A: To calculate pH of pyridine, first calculate OH- from the given data and using that find out pH.

Q: a) What is the concentration of a solution prepared by mixing 35.0 mL of o.10 Macetic acid with 15.0…

A: a) Given : Concentration of acetic acid i.e HC2H3O2 taken = 0.10 M Volume of HC2H3O2 solution taken…

Q: The diprotic acid H₂A has Ka1 = 1.58*10-5 and Ka2 = 1.47*10-6. If the initial concentration of H₂A…

Q: At 55°C aniline, CH NH₂, has a Kb = 8.2 *10-1⁰ What is the pH of a 0.035M solution in water?…

A: Givenconcentration of aniline = 0.035 Mthe Kb value of aniline = Calculate the pH of solution.

Q: My Questions b X VCU SONA FAFSA: Apply f X + X edugen/Iti/main.uni Return to Blackboard S Kime,…

A: Given that the pH of snow or rain is 4.0 . If the pH value is less than 7, then it will be acidic.…

Q: [References] Calculate (OH], H*], and the pH of 0.38 M solutions of each of the following amines (K,…

Q: What volume (in mL) of 9.2 M HCIO4 would be required to make 500.0 mL of a solution with a pH of…

A: The pH of a solution is represented by the following relation: pH=-log[H+] Where [H+] is the…

Q: Find the hydroxide ion concentration of a HBr solution with a pH of 4.75. *Hint use Kw [OH-] =…

A: The pH of a solution is the negative logarithm of hydrogen ions. The pOH of a solution is the…

Q: In a dilute sodium bicarbonate solution, [H] = 1.5 x 108 M. Without using a calculator, what integer…

A: The approximate pH of the solution is 8.

Q: NAME 6. GIVEN: Where X, Y and Z are polyatomic ions.. Acids K, @25°C) HX 5 x 104 HY 6 x 10 HZ 8 x…

A: (a) Since Ka value of HY is minimum so it is very less dissociated hence HY has highest…

Q: Which of the following statements is/are true? (Select all that apply) OThe higher the concentration…

Q: Question 5 The Ka of a weak acid HA at 25 °C is 9.6 x10-8. What is the pH of a 1.5 M solution of the…

A: Ka of weak acid HA=9.6×10^-8 Concentration of acid =1.5M pH of acid=? Percent ionization of…

Question

Expert Solution

Step 1

It's a multiple question type.

Given information,

(1) [Propanoic acid] = 0.10 M

K_a for propanoic acid = 1.3*10^-5

(2) [ethylamine] = 0.050 M

K_b for ethylamine = 6.4*10^-4

Step by step

Solved in 3 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Similar questions

Calculate the pH at 25 °C of a 0.62M solutlon of ethylammonlum bromide (C,H,NH,Br). Note that ethylamine (C,H,NH,) is a weak base with a p K, of 3.19. Round your answer to 1 decimal place. dlo pH Ar Explanation Check O 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy Accessibility V i 3:47 9 0 hp esc & @ # $ 8. 7 3 4 1 y e tab * 00
← < Upload Assic X 0o DESU Calcul. X https://app.101edu.co C + 40°F Sunny T Om An unknown weak acid with a concentration of 0.520 M has a pH of 5.100. What is the Ka of the weak acid? w Aktiv Chemis X Ghow to find i XUtilities-Go X (387) finding X su www.desu.ed X 75 R E HE T Q Search z|x| | VJBJN В alt Time's Up! U I M hp SDEGHI SU Delaware Sta X Log In | Fede XQ gmail-Sear: x + A G C • 1 3 G I P ctri 10 1 4 7 +/- 2 5 8 3 6 9 0 enter 7 C x 100 A 11:38 3/30/2 1
Gen Chemistry 2, Q5
What is the concentration of hydroxide ion in a 0.170 M aqueous solution of hydroxylamine, NH2OH? What is the pH? (K, = 1.1 x 10-) [OH ] = pH = Submit Answer Retry Entire Group 9 more group attempts remaining
Butyric acid (HC4H7O2) is a weak acid with the stench of rancid butter (please show full work)
pls help
Correct. What is the concentration of H* in 0.0072 MHCIO4? [H]=0.0072 Hint HCIO4 is a strong acid. Correct. pH = What is the pH of the solution? 2.14 M Correct. [OH]= 1.38E-12 What is the OH concentration in the solution? For scientific notations, use the format 1.0E-10, for example. M Assistance Used Incorrect. Compare the pH at double concentration to the pH at the original concentration. How would you expect the pH to change with an increase in [H]? By how much does the pH change if the concentration of H is doubled?
What is the pH of a 0.0100 M sodium benzoate solution? -10 K (C,H,0, ) = 1.5 10
make sure right number of sig fig