6. AlF3 is insoluble in liquid HF but dissolves if NaF is present. When BF3 is added to the solution, AlF3 precipitates. Write out chemical processes and explain them using the principles of Lewis acid-base theory. (6 points)

weathering. 6. The drinking water for Bloomington, Indiana, comes from Lake Monroe, which has a calcium concentration of 17 ppm. What is the pH of this lake? It may (or may not) help to remember that the atomic weight of calcium is 40.1 g/mol.

(1) 3. ddp tot W H. (be)(D) (s) 0 6 8. 7. 6. 2. Write the formula of the conjugate base of the Brønsted-Lowry acid, HCIO, Question 10 of 27

The Ka of the weak acid HSO4- (aq) is 1.2*10-2 Give the weak acid's conjugate base and calculate the congugate base's Kb.

Coleiro-ic Acid, HColeiro , is a new organic compound used to manufacture hypnotic drugs and some plastics. It has a Ka of 9.8x10-5 . An industrial process requires 0.25 mol/L solution of Coleiro-ic acid. a) Calculate the pH of the solution. (5) (Hint: The Coleiro in HColeiro will become an anion on the right side of the equation that you will need to write). b) What is the percent dissociation of Coleiro-ic acid?

Can you help me because I dont understand how to do step by step?

please,Don't provied handwriting solution...

8:44 1 ll 5GE Question 14 of 25 Submit Determine the pH of a 0.30M solution of HE (Ка 3D 6.8 х 10-). 1 2 3 Based on the given values, set up ICE table in order to determine the unknown. HF(aq) + H,0(1) =H;0*(aq) + F(aq) Initial (M) Change (M) Equilibrium (M) 5 RESET 0.30 6.8 x 10-4 0.15 +x -x +2x -2x 0.30 + x 0.30 - 0.30 + 2x 0.30 - 2x 6.8 x 10-4 + x 6.8 x 10-4 - х 6.8х 10-4 + 2х 6.8 x 10-4 - 2x

2.3 7 (a) Describe what happens when each of the following molecules is separately dissolved in water and illustrate with an equation in each case: (i) ethanoic acid (CH3COOH) (ii) ammonia (NH3) (b) Identify the conjugate acids and bases in the substances mentioned in question 7(a) above. (c) Explain the difference between: (i) a strong acid and weak acid and (ii) a strong base and a weak base

7:50 A14 (4th quarter) pH and po... 3.24 x 10-3 1.09 x 10-10 M 4.325 1 x 10-4 M Part B. 1. The hydrogen ion concentration in a solution is measured to be 7.84 X 10-5 M. Calculate the following: a) pH b) pOH c) [OH-], M 2. You have 500.0 mL (convert to liter by dividing by 1,000) of a 4.5 x 10-¹¹M of HNO₂ solution. a. How many grams of HNO3 are present in this solution? Step 1: Using the formula of molarity, solve for the moles of solute: Moles solute = M x L Step 2: Solve the MM of HNO3 using the periodic table of elements: Step 3: Multiply Steps 1 and 2 results to get the grams of HNO3. b. Complete the chart using the given value of the concentration of [H*]. [OH-] [H+] 4.5 x 10-¹¹M pH POH 11.76