Part A
3.41×10−2M HNO3.
Express the pH of the solution to three decimal places.
pH = _____
Part B
0.260 g of HClO3 in 2.60 L of solution.
Express the pH of the solution to three decimal places.
pH = _____
Part C
10.00 mL of 1.70 M HCl diluted to 0.520 L .
Express the pH of the solution to three decimal places.
pH =_____
Part D
A mixture formed by adding 41.0 mL of 2.5×10−2M HCl to 160 mL of 1.0×10−2M HI.
Express the pH of the solution to two decimal places.
pH = _____
pH= -log[H+]
part A
pH=-log[H+]=-log[3.41*10^-2] =1.467
part B
Moles= 0.260/molar mass of HClO3 = 0.260/84.5
Molarity= moles/volume = 0.260/84.5 *1/2.60 = 0.00118
pH=-log[H+]=-log[0.00118] =2.928
part C
Moles= 1.70*10ml = 17m moles
Molarity= moles/volume = 17m moles/520ml =0.0327
pH=-log[H+]=-log[0.0327 ] =1.485
part D
total Moles=2.5*10^-2*41ml+ 1*10^-2*160ml = 2.625m moles
Molarity= moles/volume =2.625m moles/(41+160)ml =0.01306
pH=-log[H+]=-log[0.01306 ] =1.88
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