What is the concentration of H3O+ in each of the following solutions?
a. 0.010 M HNO3
b. 0.020 M HClO4
c. 0.0150 M NaOH
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Calculate the [H+] and [OH-] of each of the following solutions. 0.010 M HCl 0.010 M H2SeO4 0.025 M KOH 0.020 M Ba(OH)2
Calculate the pH of each of the following strong acid solutions: (a) 0.0167 M HNO3, (b) 0.225 g of HClO3 in 2.00 L of solution, (c) 15.00 mL of 1.00 M HCl diluted to 0.500 L, (d) a mixture formed by adding 50.0 mL of 0.020 M HCl to 125 mL of 0.010 M HI.
Which of the following solutions would have the same boiling point as 0.040 m C6H12O6, a nonelectrolyte, in water?
0.010 m Na3PO4 in water
0.020 m CaBr2 in water
0.020 m KCl in water
0.020 m HF in water (HF is a weak acid)