A 0.005 L solution of the strong acid HClO4, has a pH of 2.50. Calculate the mass (number of grams) of HClO4 that was used to make the solution.
A 0.005 L solution of the strong acid HClO4, has a pH of 2.50. Calculate the...
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 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 =
A) A solution of HClO4 has a pH of 2.41. How many grams of HClO4 are there in 254 mL of this solution? B) How many grams of HClO4 are in 254 mL of. HClO4 solution that has twice the pH?
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 =
Calculate buffer pH after adding strong acid or strong base. Close Problem Determine the pH change when 0.064 mol HClO4 is added to 1.00 L of a buffer solution that is 0.309 M in HNO2 and 0.262 M in NO2-. pH after addition − pH before addition = pH change =
1. For the strong acid solution 0.0098 M HClO4, determine [H3O+] and [OH−]. Express your answers using two significant figures. Enter your answers numerically separated by a comma. For this solution determine pH. 2. For the strong acid solution 7.5×10−3 M HBr, determine [H3O+] and [OH−]. For this solution determine pH. 3. For the strong acid solution 3.77×10−4 M HI, determine [H3O+] and [OH−]. 4. For this solution determine pH. For the strong acid solution 0.0978 M HNO3, determine [H3O+]...
Calculate pH in a) a 0.005 M solution of HCl, and b) a 0.005 M solution of acetic acid and explain why the pH values are different.
16. A 1.00 L solution of strong acid with a pH of 5.00 is added to a 1.00 L solution of a strong acid with a pH of 4.00. What is the final pH of the mixture? A) 4.00 D) 3.96 B) 5.00 E) 4.26 C) 4.50 16. A 1.00 L solution of strong acid with a pH of 5.00 is added to a 1.00 L solution of a strong acid with a pH of 4.00. What is the final...
Calculate the pH of each of the following strong acid solutions. Calculate the pH of each of the following strong acid solutions. (a) 0.00696 M HI pH = (b) 0.719 g of HCl in 29.0 L of solution pH = (c) 49.0 mL of 2.10 M HI diluted to 3.40 L pH = (d) a mixture formed by adding 87.0 mL of 0.000520 M HI to 47.0 mL of 0.000860 M HCI pH =
Part 1.) Calculate the pH of each of the following strong acid solutions. (a) 0.00555 M HClO4 pH = (b) 0.314 g of HBrO4 in 21.0 L of solution pH = (c) 39.0 mL of 3.50 M HClO4 diluted to 1.90 L pH = (d) a mixture formed by adding 59.0 mL of 0.00582 M HClO4 to 16.0 mL of 0.00676 M HBrO4 pH = Part 2.) Using values from Appendix C of your textbook, calculate the value of Keq...