IV. Complete the table by computing for the missing pH, pOH, [H*], and [OH-] 1. 2. 3. 4. 5. [H+] 4.73x10-10 [OH-] 8.53x10-7 pH 3.78 7.05 POH 12.24 Acidic or basic

Complete the table: H3O+ OH1- pH acidic/basic/neutral? 4.45x10-9 M         2.7x10-3 M         6.57

Determine [OH- ] in a solution at 25°C if pH = 10.50. a) 3.2 × 10-11 M         d) 7.1 × 10-8 M b) 3.2 × 10-4 M          e) 8.5 × 10-7 M c) 1.1 × 10-2 M

Can you help me step by step with number 13, please? Can you explain it to me?

A 0.063 M solution of a base has a pH of 11.40. a What are the hydronium and hydroxide ion concentrations of this solution? [H3O+] = [ [OH-] = M M

Which of the following does NOT describe an acidic solution?????a. the pH is less than 7 b. the [OH-] is greater than 1 x 10-7 M c. the [H3O+] is greater than [OH-] d. the [OH-] is 6.0 x 10-10 M.

Question: Explain the process of self-ionisation/autoionisation of water molecules. The points should be taken: a. You have to show an equation for the self-ionization of water. b. How is water both an acid and a base? c. Identify the conjugate acid-base pairs d. Distinguish the condițions between (H3O] [OH], [HO)> [OH] and [H3O)< [OH]

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Determine the [OH-] in a solution with a pH of 6.008.  Your answer should contain 3 significant figures as this corresponds to 3 decimal places in a pH.

Question 2 Which statement is true if an aquous solution is not neutral at 25°C. ? Explain your reasoning in a separate sheet a. [OH-] = 1.0 x 10-7 M O b. [H3O+][OH-] = 1.0 × 10-14 OC. [H30¹] = [OH-] Od. [H3O+] = 1.0 x 10-7 M O e. NIZA 336 e. [H3O+][OH-] = 1.0 × 10-7 Moving to another question will save this response. 45,836 MAY 23 1 tv