A patient's urine sample gave a pH reading of 8.2. What is the value of #[H_3O^+]# in this?
This is a pretty straightforward problem that can be solved by using the equation
#color(blue)(["H"_3"O"^(+)] = 10^(-"pH"))#
In your case, the concentration of hydronium ions,
#["H"_3"O"^(+)] = 10^(-8.2) = 6.31 * 10^(-9)"M"#
Interestingly enough, the normal pH range for urine lies between
By comparison, the normal pH range for blood is much less susceptible to variation. For a healthy individual, blood pH ranges from
This pH range is controlled by the carbonic acid/bicarbonate buffer, one of the body's main buffer systems.