8) Calculate the [H30+) and the pH of a 0.021 M HNO3 solution. A) 4.8 x...
6) Calculate the pH of a 0.021 M NaCN solution. [K (HCN) 4.9 x 1010] 6) a A) 5.49 B) 1.68 C) 3.18 D) 7.00 E) 10.82
Calculate the [OH-] and the pH of a solution with an [H+] = 4.8 x 10-6 M at 25 °C.Calculate the [H+] and the pH of a solution with an [OH-] = 8.8 x 10-13 M at 25°C. Calculate the [H+] and the [OH-] of a solution with a pH = 11.04 at 25°C.
What is the equilibrium pH of a 0.515 M solution of H3PO4 (aq)? (Ka1 = 7.5 × 10–3 , Ka2 = 6.2 × 10–8 , Ka3 = 4.8 × 10–13) a. 1.23 b. 3.75 c. 12.32 d. 6.30 e. 7.21
3a. Calculate the pH of a 7.8x10 * M HCl solution. 3b. Is this solution acidic, basic or neutral? 4a. Determine the pH of 1.3 x 10 M NaOH. 4b. Is this solution acidic, basic or neutral? 5a. A 0.1 M NaHCO3 solution has a pH of 8.400. What is the [H3O'? 5b. Is this solution acidic, basic or neutral? 6. Determine whether the following statements are true or false regarding a 0,010 M solution of the strong acid HNO3:...
1) An Arrhenius acid is defined as a substance which: A) increases [H+] when placed in water C) decreases [H+] when placed in water B) acts as proton acceptor in any system D) acts as proton donor in any system 2) Which of the following is a correct balanced equation for the neutralization reaction that occurs between Al(OH)3 and HCl(aq)? A) Al(OH)3 + HCl(aq) → AICI3 + H20 B) Al(OH)3 + 3 HCI (aq) → AICI3 + H+ + OH-...
Saved Calculate the pH of a solution that has [H30*)= 1.0 x 10-6 M. Multiple Choice pH = 1.00 pH = 7.00 pH = 6.00 < Prev 45 of 60 !!! Next > search O PRE
PROBLEMS 1) Acids and bases: Calculate the following a) [H30] in a 0.500 M solution of HCl b) pH of a 0.100 M solution of HCI c) pH of a 0.100 M solution of HNO3 d) [OH] in a 0.500 M solution of HClnote, for this you need to use Kw e) pH of a 0.100 solution of NaOH (also need to use some form of Kw here)
A) calculate the ph of a 0.028 M HNO3 solution B) Calculate the pH of a 0.028 M solution of benzoic acid (Ka=6.5x10^-5)
1. Calculate the pH of each solution. a) [H20*=1.7x10-8 M b) [H3O+]=1.0x10-?M c) [H30+1=2.2x10M 2. Calculate the pH of each solution. a) [OH-]=1.9x10-7M b) [OH"]=2.6x10-8 M c) [OH"]=7.2x10-'M 3. Calculate the pH of each solution: a) 1.28x10-M KOH b) 1.54x10-*M Sr(OH)2
Calculate the pH of a solution containing 0.0334 M potassium hydrogen fumarate and 0.021 M dipotassium fumarate. The Ka values for fumaric acid are 9.50 × 10-4 (Ka1) and 3.30 × 10-5 (Ka2).