For each of the following cases, decide whether the pH is less than 7, equal to 7, or greater than 7. a. 85 mL of 0.30 M H2S is mixed with 85 mL of 0.60 M NaOH. O The pH of the solution is less than 7. O The pH of the solution is equal to 7. O The pH of the solution is greater than 7. b. 70. mL of 0.65 M acetic acid, CH3 CO;H is mixed with 70. mL of 0.65 M NAOH. O The pH of the solution is less than 7. O The pH of the solution is equal to 7. O The pH of the solution is greater than 7. c. 80. mL of 0.65 M H2SO4 is mixed with 80. mL of 0.65 M NAOH. O The pH of the solution is less than 7. O The pH of the solution is equal to 7. O The pH of the solution is greater than 7.

Which is a conjugate acid base pair in the following equation?H 3PO 4 + H 2O  H 3O +1 + H 2PO 4 -1 What is the pH of a solution whose H +1 concentration is 4.0 X 10 -9?   a. 4.0     b. 8.4     c. 3.6     d. 9.0     What is the boiling point of a 2.0 m aqueous solution of sodium chloride?(The boiling point elevation constant for water is 0.512 °C/m.)    please answer all

A sample of water from a stream has [H3O*]=3.1 × 10-9 M. Which statement below accurately describes this water sample? A. The water sample is acidic. B. The water sample is a basic solution. C. The pOH of the water sample is 8.50. D. pH of the water sample is much les than 7.0. E. The pH of the water sample is 7.5.

0.100 moles of each substance is dissolved in 1.0 L of water. Decide if each is an acid or a base and if it is strong or weak. Circle which description best describes the pH of the solution.

1. The equilibrium constant, K, for a monoprotic acid (propionic acid) is 1.3 x 10-5. Which of the following is the correct value of K, for the propionate ion, the conjugate base of propionic acid? a. 1.3 × 10⁹ b. 1.3 × 10-19 c. 7.7 x 104 d. 1.3 × 10-5 e. 7.7 x 10-10 -. Which of the following expressions correctly describes the equilibrium constant K, for the reaction given below? 4 NH3(g) +5 O₂(g) 4 NO(g) + 6 H₂O(g) a. Kc = b. Kc = c. Ke= d. Ke= e. Kc = [NO₂][H₂O] [NH3][0₂] 4[NH3]+5[0₂] 4[NO]+6[H₂0] [NO][H₂O16 [NH,[0₂] [NH₂] [0₂] [NO][H₂O] 4[NO]+6[H₂0] 4[NH3]+5[0₂]

A 0.0010 M acetic acid (CH3COOH) solution produces 1.2 x 10-4 M of acetate ions (CH3CO0'). What is the pH of the acetic acid solution? Select one: a. 3.92 b. 10.08 c. 11.00 d. 3.00

The pH of a 0.030 M formic acid (HCOOH) solution is 2.63. If 0.030 M sodium formate (NaHCOO) is added, which of the following statements will be true?  A. the pH will decrease  B. the equilibrium position shifts to the left C. the [H3O+] will increase D. the [HCOOH] will decrease

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A 1.0-liter solution contains 0.25 M HF and 0.41 M NaF (Ka for HF is 7.2 x 10-4). What is the pH of this solution? O a. 3.36 O b. 10.64 O c. 2.93 O d. 3.14 O e. 0.21

Question Completion Status: QUESTION 20 A solution has a pH of 5.4. What is its pOH? O a.-8.6 O b.-5.4 O c. 5.4 O d. 8.6 QUESTION 21 A sodium hydroxide solution at room temperature has a pH of 11.40. What is its [OH]? O a. 4.0 × 10-26 M O b.4.0 × 10-12 M OC 2.5 × 10-3 M O d. 2.5 x 1011 M QUESTION 22 In the process of autionization of water, as seen below: 2 H₂0 (1) H3O+ (aq) + OH (aq) O hydronium (H30*) is acting as the base Owater is the acid Owater is both the acid and the base O water is the base Click Save and Submit to save and submit. Click Save All Answers to save all answers.