How many grams of NaA (57.93 g/mol) would need to be added to 590 mL of 1.17 M HA to produce a solution with a pH equal to 5.8? Report your answer to the tenths place. The Ka of the weak acid (HA) is 6 × 10-7.     Please explain each step, i want to learn.

What is the pH of a solution that is 0.25 M CH3NH2 (methylamine) and 0.43 M CH3NH3Cl (methylammonium chloride)? (Assume Kw is 1.0  10-14.)

What is the pH of a solution that is 0.200 M ammonia (NH3) and 0.150 M ammonium chloride (NH4Cl)?  The Kb of NH3 is 1.8 × 10-5   Part D:  What is the pKa of NH4+? Report your answer to two digits past the decimal.

A certain base has a Kb of 7.8 × 10-6 . What concentration of the base will produce a pH of 11.32?

Many important biochemicals are organic acids, such as pyruvic acid (pka = 2.5) and lactic acid (pka = 3.86). For each acid, draw a simple titeation curve, and label the pKa. Draw an arrow where the line crosses pH 3 for each acid? Calculate the percentage of acid and conjugate base for both at pH 3..

Which of the following statements is TRUE? Select one: A solution with a pOH of 4 is basic.   It is not possible to have a pH outside the range 0 - 14.   A 1 M solution of HCl will have a higher pH than a 1 M solution of HF. Carbonic acid (Ka = 4.3 × 10-7) is a stronger acid than oxalic acid (Ka = 5.9 × 10-2). Basic solutions don't contain any H3O+ ions.

Answer the 2 questions below: Determine both the H and the pH in a 0.0088 M solution of HCIO, at 25 °C? (H*)= Type your answer here M pH = Type your answer here Determine both the OH and the pOH in a 0.0032 M solution of Ba(OH)2at 25 °C? OH]= Type your answer here M pOH = Type your answer here Unanswered 梦 $ a hp prt sc delete backspace

11 Ammonia and oven cleaner are both bases. Their [H+] values are 1.3 × 10¹¹ mol/L and 6.3 × 10-¹4 (a) Find the pH for ammonia. (b) Find the pH for oven cleaner. (c) Which substance is more basic? Part: 0 / 3 Part 1 of 3 (a) Find the pH for ammonia. The pH for ammonia is approximately X 3 mol/L, respectively.

Consider 1M solutions of each of the following acids (with their Ka values). Which solution would have the highest pH? HCN, 4.9 x 10-10 HCIO, 2.9 x 10-8 H202, 2.4 x 10-12 HF, 3.5 x 104

A certain weak acid, HAHA, has a Ka�a value of 4.4×10−7.  Calculate the percent ionization of HAHA in a 0.10 M� solution. Express your answer as a percent using two significant figures.