2 . Without calculation , which solution in each pair has the higher pH?
a) 0.10 M HNO3 or 0.10 M HNO2 ? _______________________
b) 0.10 M NaNO3 or 0.10 M NaNO2 ? _______________________
c) solution that is 0.10 M NaNO2and 0.10 M HNO2 or a solution that is 0.10 M HNO2 (only)? __________________
2)
a) weaker the acid higher the pH
0.1M HNO2 has higher pH
b) NaNO2 has higher pH then NaNO3
c) mixture of NaNO2 and HNO2 has higher pH
2 . Without calculation , which solution in each pair has the higher pH? a) 0.10...
indicate which solution in each pair has the lower pH -/0.5 POINTS No Marks. To determine what portion of the question you have correct, check question score at the top of the assignment. Indicate which solution in each pair has the lower pH. lower pH -Select--- 0.1 M HCIO 0.2 M HCIO2 0.1 M NaClO2 0.2M NACIO --Select- 0.1 M HF 0,1 M HNO2 Select 0.1 M NaOH water
Indicate which solution in each pair has the lower pH. (a) 0.2 M NaClO2 or 0.1 M NaClO2 (b) 0.1 M HClO2 or 0.2 M HClO2 (c) water or 0.1 M NaOH (d) 0.1 M HF or 0.1 M HNO2
Which solution would have the higher pH? 0.10 M NH_3(k_b = 1.8 times 10^-5) 0.10 M NH_4 Cl both would have the same pH. Which solution would have the lower pH? 0.10 M KNO_3 0.10 M Fe (NO_3)_3 both have the same pH.
which one of the following is a buffer solution? a) 0.40 M HCN and 0.10 KCN b) 0.20 CH3COOH c) 1.0 M HNO3 and 1.0 NaNO3 d) 0.10 M KCN e) 0.50 M HCl and 0.10 NaCl
a. How many moles of hydroxide ion are in a 100.0 L solution that has a pH of 10.00? b. When the concentration of hydronium ion, [H3O+],decreases by a factor of 1000, what happens to the pH? c. Which solution should have the greatest concentration of H3O+, and which should have the lowest pH? (One is a strong acid and one is a weak acid.) 0.10 M HNO2 0.10 M HNO3
Determine the pH of the resulting solution as each change is made step-wise (assume volume is additive along the way): a. 25.00 mL water placed into 600 mL beaker. b. 3.00 mL of 1.00 M HNO3 is added. c. 3.00 mL of 1.00 M LiOH is added. d. 42.00 mL of 1.00 M HNO2 is added. e. 22.00 mL of of 1.00 M LiNO3 is added. f. 15.00 mL of 1.00 M NaNO2 is added. g. 1.00 mL of 1.00...
Which one of the following mixtures is a buffer solution? 0.40 M HCN and 0.10 KCN 0.20 M CH3COOH 1.0 M HNO3 and 1.0 M NaNO3 0.10 M KCN 0.50 M HCl and 0.10 NaCl
Post-Lab Assignment: pH and Buffers 1. A buffer is prepared from a weak acid with a Ka - 7.1 x 104 and its conjugate base. a. What pH would provide maximum buffer capacity? b. What would be the buffer range for this acid? (Your answer should show the lowest and the highest pH that would provide a reasonably effective buffer.) 2. If you were provided with a 0.1 M solution of an unknown weak acid and a 0.1 M solution...
1. If a 0.10 M solution of an acid has a pH of 4.5, using your data and graph from goal 2, what would be the predicted pH of a 0.10 M solution of the conjugate and why? Goal #2 Conjugate Acid Base Pair pH of Acid pH of Base HCl/Cl- 1.60 4.94 Formic Acid/Formate 2.49 6.72 Propionic Acid/Propanoate 3.21 7.67 Ammonium/Ammonia 5.89 11.10 this is the data from goal 2
2&3 please show work Question 2) 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Determine the pH of the solution before the addition of any HNO3. The Kb of NH3 is 1.8x 10-5 A) 4.74 B) 9.26 C) 11.13 D) 13.00 E) 12.55 Answer "Calculation: Question 3) Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M HCHO2 with 100.0 mL of 0.20 M LICHO2. The Ka for HCHO2 is 1.8...