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QUESTION

# Solution A has a a hydronium ion concentration of 1.3 x 10^-3 M. Solution B has a hydroxide ion concentration of 4.5 x 10^-8M. Calculate the pH of solutions A and B Show all calculations?

pH_A = 2.89

pH_B = 7.44

By definition, pH = -log_10[H_3O^+].

pH_A = -log_10[1.3xx10^-3]=2.89

pOH_B = -log_10[4.5xx10^-8]=7.44

Since pH+pOH=14, pH_B = 6.56

What does it mean when we say log_AB=c?

Can you tell me the values of log_(10)10 and log_(10)100?