both 5 and 6 please 5) What is the H30* concentration to the correct number of...

Question

Question

both 5 and 6 please
5) What is the H30* concentration to the correct number of significant figures for solutions with the following pH values? (a

Answer 1

Answer #1

SOLN 5

pH = -log (H₃O⁺)

hence H₃O⁺ = 10^-pH

(a) at pH = 0 H₃O⁺ = 10^-0 =1.00 M

(b) at pH =7.00 H₃O⁺ = 10^-7 =1.00 * 10^-7 M

(c) at pH = 2.63 H₃O⁺ = 10^-2.63 = 0.00234 M

(d) at pH = -0.42 NOT POSSIBLE (assuming solvent to be water)

(e) at pH =11.21 H₃O⁺ = 10^-11.21 =6.16*10^-12 M

According to HOMEWORKLIB POLICY only 1 question per post is allowed. please post the rest question seperately.

PLEASE LEAVE THE POSITIVE FEEDBACK IF YOU LIKE THE SOLUTION

Answer 2

Similar Homework Help Questions

IWCI. 5) What is the H30 pH values? (a) 0.00 concentration to the correct number of...

IWCI. 5) What is the H30 pH values? (a) 0.00 concentration to the correct number of significant figures for solutions with the following (b) 7.00 (c) 2.63 (d) - 0.42 (e) 11.21 6) (a) Calculate the pH of a buffer solution that is 0.45 M in NH4Cl and 0.15 M in NH3. (b) How would you prepare an NH4Cl-NH; buffer that has a pH of 9.00? (The Kb for NH; is 1.8 x 10%)
AUSWC. 5) What is the H30* concentration to the correct number of significant figures for solutions with the follow...

AUSWC. 5) What is the H30* concentration to the correct number of significant figures for solutions with the following pH values? (a) 0.00 (b) 7.00 (C) 2.63 (d) -0.42 (e) 11.21 (a) Calculate the pH of a buffer solution that is 0.45 M in NH4Cl and 0.15 M in NH3. (b) How would you prepare an NH4Cl-NH3 buffer that has a pH of 9.00? (The Kb for NH3 is 1.8 x 10)
Answer Both questions please. (11) (6 points) What is the HO. concentration to the correct number...

Answer Both questions please. (11) (6 points) What is the HO. concentration to the correct number of significant figures for solutions withthe following pH values? (a) pH-0.00 (b) pH-7.00 (pH--0.20 ID) (4 points) Calculate the pH of 0.16 M KOH solution.

please answer 1 and both parts of 2 1. Which one of the following sets of...

please answer 1 and both parts of 2 1. Which one of the following sets of compounds is not characteristic of a buffer? a. HNO3 with NaNO b. NaH POwith Na2HPO: C. NH; with NHACI d. CH3COOH with NaCH3COO 2. What is the pH of the following buffer solutions? a. 0.45 M NH3 and 0.55 M NH-CI. K. (NH3) = 1.8 x 105 b. 0.36 M HCOOH and 0.55 M KHCOO. K. (HCOOH) = 1.8 x 104
I need help with number 9 please 9. Using the experimental data for pH and the...

I need help with number 9 please 9. Using the experimental data for pH and the concentration of the solutions, calculate the K, and Ky for each salt. (SHOW YOUR WORK.) Solution Value of K, or Kb 0.1 ZnCl2 0.1 KAl(SO4)2 0.1 NHACI 0.1 NaC2H302 Value of K, or Kb Solution 0.1 Na2CO3 Part B. Buffer solutions and pH 10. Mass of NaC2H307-3H203.316 11. Measured pH of original buffer solution 4 0 12. Measured pH of buffer + HCI_4.2 13....
Be sure to answer all parts. What is the H30+ and the pH of a benzoic...

Be sure to answer all parts. What is the H30+ and the pH of a benzoic acid-benzoate buffer that consists of 0.17 M C6H3COOH and 0.35 M C6H3COONa? (K, of benzoic acid = 6.3 x 10-5) Be sure to report your answer to the correct number of significant figures. [H30+]= * 10 M pH =

I need help with #4. "show by calculation why acetic acid (Ka = 1.8 X 10^-5), when combined with NaC2H3O3 as a buffe...

I need help with #4. "show by calculation why acetic acid (Ka = 1.8 X 10^-5), when combined with NaC2H3O3 as a buffer, will not produce a pH o 9.00" 1. What is the pH of a 1.0L buffer that is 0.10 M in Naz HPO4 and 0.15 M in NaH2PO4? Write the equilibrium reaction equation and corresponding Ka expression for the buffer. K for H2PO4 is 6.2 X 108 2. A 10.00 mL sample of 0.300 M NH3 is...
A certain weak base has a K of 7.50x107. What concentration of this base will produce...

A certain weak base has a K of 7.50x107. What concentration of this base will produce a pH of 10.23? Number 00017 NH3 is a weak base (Kb = 1.8 x 10-5) and so the salt NH4Cl acts as a weak acid. What is the pH of a solution that is 0.069 M in NH4Cl at 25 °C? Number pH-
4.13 Just as pH is the negative logarithm of [H3O+], pKa is the negative logarithm of...

4.13 Just as pH is the negative logarithm of [H3O+], pKa is the negative logarithm of Ka, pKa=−logKa The Henderson-Hasselbalch equation is used to calculate the pH of buffer solutions: pH=pKa+log[base][acid] Notice that the pH of a buffer has a value close to the pKa of the acid, differing only by the logarithm of the concentration ratio [base]/[acid]. Part B How many grams of dry NH4Cl need to be added to 2.10 L of a 0.400 M solution of ammonia,...

QUESTION 6 What is the pH of a solution with a hydronium (H30) concentration of 6.3...

QUESTION 6 What is the pH of a solution with a hydronium (H30) concentration of 6.3 * 10-5 M.