pH = 10.2
pOH = 14 - pH = 14 - 10.2 = 3.8
[OH-] = 1 x 10-pH = 1 x 10-3.8 = 1.58 x
10-4 M
[NaOH] = [OH-] = 1.58 x 10-4 M
moles of NaOH = molarity of NaOH x volume of NaOH = 1.58 x 10-4 x 5.40 = 8.56 x 10-4 mol
mass of NaOH solute = moles of NaOH x molar mass of NaOH = 8.56 x 10-4 x 40 = 0.034 g
mass of 15% NaOH solution = mass of NaOH salute / 15% = 0.034 / 0.15 = 0.227 g
volume of 15% NaOH = mass of 15% NaOH solution / density of 15% NaOH solution
= 0.227 g/ 1.116 g/ml = 0.203 ml
What volume of a 15% by mass NaOH, which its density is 1.116g/mL, should be used...
Part A What volume of a 150% by mass NaOH solution, which has a density of 1.116/mL should be used to make 465 L of an NaOH solution with a pH of 1027 Express your answer to one significant figure and include the appropriate units. Value Units Submit Previous Answers Request Answer X Incorrect: Try Again: 4 attempts remaining
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