Calculate the pH of each of the following strong acid solutions. (a) 0.00438 M HClO4 pH = (b) 0.579 g of HCl in 21.0 L of solution pH = (c) 59.0 mL of 3.90 M HClO4 diluted to 4.50 L pH = (d) a mixture formed by adding 69.0 mL of 0.00809 M HClO4 to 78.0 mL of 0.00483 M HCl pH =
Calculate the pH of each of the solutions and the change in pH to 0.01 pH units caused by adding 10.0 mL of 2.27-M HCl to 670. mL of each of the following solutions. a) pH of water before mixing, after mixing and pH change b) 0.152 M C2H3O21- pH before mixing, after mixing and pH change c) 0.152 M HC2H3O2 pH before mixing, after mixing and pH change. d) a buffer solution that is 0.152 M in each C2H3O21-...
Determine the pH of each solution. Part A 4.6×10-2 M HI Part B 8.43×10−2 M HClO4 Part C a solution that is 4.3×10−2 M in HClO4 and 5.6×10−2 M in HCl Part D a solution that is 1.11% HCl by mass (Assume a density of 1.01 g/mL for the solution.)
Which of the following solutions has the lowest pH? 0.002-M HClO4, 0.20-M CH3COOH, 0.02-M HCl, 2.0-M NaCl, 0.200-M HCOOH (I asked this before but I am unsure if the answer I received is correct so I am resubmitting it.)
Calculate the pH of each of the following strong acid solutions. (a) 0.00471 M HClO4 pH = (b) 0.329 g of HBr in 16.0 L of solution pH = (c) 65.0 mL of 7.50 M HClO4 diluted to 4.60 L pH = (d) a mixture formed by adding 54.0 mL of 0.00155 M HClO4 to 47.0 mL of 0.00191 M HBr pH =
For each strong acid solutions, determine [H3O+],[OH−], and pH. 1. 0.21 M HCl. 2. 2.6×10-2 M HNO3 3. a solution that is 5.1×10−2 M in HBr and 1.7×10−2 M in HNO3 4. a solution that is 0.675 % HNO3 by mass (Assume a density of 1.01 g/mL for the solution.)
Calculate the pH of each of the following strong acid solutions. (a) 0.00890 M HI pH = (b) 0.901 g of HClO4 in 28.0 L of solution pH = (c) 17.0 mL of 3.70 M HI diluted to 4.70 L pH = (d) a mixture formed by adding 12.0 mL of 0.00655 M HI to 72.0 mL of 0.000920 M HClO4 pH =
What is the pH value of the following composition of solutions? a) 1 mL 0.10 M HC2H3O2 + 99 mL H2O b) 5 mL 0.10 M HC2H3O2 + 5 mL 0.10 M HCl c) 0.10 M H3PO4 d) 0.10 M NH3 e) 0.10 M NH4NO3 f) 50 mL 0.10 M NH3 + 50 mL 0.10 M NH4NO3 g) 10 mL Solution (h) + 6 mL H2O h) 10 mL Solution (h) + 5 mL H2O + 1 mL 0.10 M...
Determine (OH"], [HT], and the pH of each of the following solutions. a. 2.9 M KCI [OH-] = [H+] = pH = b. 1.0 M KC2H302 (KA = 1.80 x 10-5) [OH"]= M (H+) = pH = Submit Answer Try Another Version 6 item attempts remaining [References] A 10.0-ml sample of an HCl solution has a pH of 2.00. What volume of water must be added to change the pH to 4.9? Volume = ml Submit Answer Try Another Version...
For each strong acid solutions, determine [H3O+],[OH−], and pH. 1. a solution that is 6.8×10−2 M in HBr and 2.4×10−2 M in HNO3 2. a solution that is 0.610 % HNO3 by mass (Assume a density of 1.01 g/mL for the solution.)