The pKa of NH3 is estimated to be 35. Its conjugate base, the amide ion (NH2), can be isolated as an alkali metal salt, such as sodium amide (NaNH2). Calculate the pH of a solution prepared by adding 0.100 mol of sodium amide to 1.00L of water. Round to two decimal places. pH = %3D Check Answer You can check your answer 4 more times before the question is locked.

The pKa of NH3 is estimated to be 35. Its conjugate base, the amide ion (NH2), can be isolated as an alkali metal salt, such as sodium amide (NaNH2). Calculate the pH of a solution prepared by adding 0.100 mol of sodium amide to 1.00L of water. Round to two decimal places. pH = %3D Check Answer You can check your answer 4 more times before the question is locked.

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

Similar questions

Predict the pH (> 7, < 7, or = 7) for solutions containing the following salts. Include a reason as to why you chose what you chose (Ka & Kb values)RbBrKNO2NH4CNFeCl3
hello please help me with part a,b, and c. handwritten solutions are more accurate than typed. Using tabulated Ka and Kb values, calculate the pH of the following solutions.Answer to 2 decimal places. 1a) A solution containing 3.3×10-1 M HCOOH and 3.0×10-1 M HCOONa. 1b) 1000.0 mL of solution containing 19.0 g of HOCl and 10.0 g of NaOCl. 1c) A solution made by mixing 95.00 mL of 0.900 M HOCl with 50.00 mL of 0.800 M NaOH.
U16V1 Question 2 Homework • Unanswered Fill in the Blanks Type your answers in all of the blanks and submit What is the pH of an aqueous solution with [H+] = 3.50x10-M? pH = Type your answer here What is the pH of an aqueous solution with (H*) = 5.20x10-M? pH = Type your answer here Unanswered A Submir [ Fullscreen 10:55 PM 5/8/2021 Cop 74 40 elete home num - backspace lock liome enter pause Tshift end
Apr 1st, A 10.4 g sample of methylammonium chloride, CH3NH3CI, is dissolved in enough water to make 250 mL of solution. Calculate the pH. Use Table 15.4 for relevant Kb values. Type your numeric answer and submit
Complete the table below. Be sure each of your answer entries has the correct number of significant digits. You may assume the temperature is 25 °C. conjugate acid conjugate base formula K. formula K, HONH, -8 1.1 x 10 CH, NH, -4 4.4 x 10 do H,CO, -7 4.5 x 10 Explanation Check Terms of Use Pacy Center Accessby 2022 McGraw HLLC ARights Reserved IA cearch 99+ 724 AS ZenBook F12 IN Pt Sc F1O Insert F9 F6 F7 F8 F4 F5 & 8. 24 4. 5
Calculate H3O+| for a solution with a pH of 7.59. Express the concentration using two significant figures. ? HẢ [H3O*] = Value Units Submit Request Answer Provide Feedback P Pearson Copyright © 2022 Pearson Education Inc. All rights reserved. Terms 80 F2 000 F3 F4 F5 F6 F7
< Which of the following solutions would be expected to have a pH of 7.00? Weak Acid HCN HNO₂ HIO HBrO C6H5COOH Ka 4.9 x 10-1⁰ 4.5 x 10-4 2.3 x 10-¹1 2.5 x 10-⁹ 6.3 x 10-5 Question 4 of 11 Tap here or pull up for additional resources Weak Base HONH, NH3 CoHsNH, H₂NNH₂ C5H5N A) CSIO B) NaF C) LICIO3 D) KNO₂ Submit
Enough of a monoprotic acid is dissolved in water to produce a 0.0040 M solution. The pH of the resulting solution is 3.50. What is the Ka of the acid? Be careful any approximations you may implicitly assuming are true. A) 0.0790 B) 40,000 C) 2.500 × 10-5 D) 2.715 × 10-5 E) 36,832
PassignmentProblemiD=182385374 pl = H-C-H Provide Feedback H.
A chemist dissolves 635. mg of pure potassium hydroxide in enough water to make up 80. mL of solution. Calculate the pH of the solution. (The temperature of the solution is 25 °C.) Round your answer to 2 significant decimal places. x10 Explanation Check O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center Accessibility 1:00 P 4/1/202. 80 F Cloudy DELL PgDn Delete PrtScr Insert F12 F10 F11 F8 F9 F7 Num Lock 69 F5 F6 F3 F4 F2 F1 Backspace & $ % @ 2# 7 8. 3 4 2
I need help to calculate this data pleasethanks a lot
The pH of a 1.93 M solution of a weak base B is measured to be 10.87 Determine Kb of the base Determine Ka of the weak bases's conjugate acid, HB+ Determine [H+] in a 2.00 M solution of the chloride salt, HBCl Determine the pH of a 2.00 M solution of the chloride salt, HBCl