pH and pOH Quiz

PDF page 777: As discussed earlier, hydronium and hydroxide ions are present both in pure water and in all aqueous solutions, and their concentrations are inversely proportional as determined by the ion product of water (Kw). The concentrations of these ions in a solution are often critical determinants of the solution’s properties and the chemical behaviors of its other solutes, and specific vocabulary has been developed to describe these concentrations in relative terms. A solution is neutral if it contains equal concentrations of hydronium and hydroxide ions; acidic if it contains a greater concentration of hydronium ions than hydroxide ions; and basic if it contains a lesser concentration of hydronium ions than hydroxide ions. A common means of expressing quantities that may span many orders of magnitude is to use a logarithmic scale. One such scale that is very popular for chemical concentrations and equilibrium constants is based on the p-function, defined as shown where “X” is the quantity of interest and “log” is the base-10 logarithm: pX = −log X

PDF page 777: As discussed earlier, hydronium and hydroxide ions are present both in pure water and in all aqueous solutions, and their concentrations are inversely proportional as determined by the ion product of water (Kw). The concentrations of these ions in a solution are often critical determinants of the solution’s properties and the chemical behaviors of its other solutes, and specific vocabulary has been developed to describe these concentrations in relative terms. A solution is neutral if it contains equal concentrations of hydronium and hydroxide ions; acidic if it contains a greater concentration of hydronium ions than hydroxide ions; and basic if it contains a lesser concentration of hydronium ions than hydroxide ions. A common means of expressing quantities that may span many orders of magnitude is to use a logarithmic scale. One such scale that is very popular for chemical concentrations and equilibrium constants is based on the p-function, defined as shown where “X” is the quantity of interest and “log” is the base-10 logarithm: pX = −log X

PDF page 777: As discussed earlier, hydronium and hydroxide ions are present both in pure water and in all aqueous solutions, and their concentrations are inversely proportional as determined by the ion product of water (Kw). The concentrations of these ions in a solution are often critical determinants of the solution’s properties and the chemical behaviors of its other solutes, and specific vocabulary has been developed to describe these concentrations in relative terms. A solution is neutral if it contains equal concentrations of hydronium and hydroxide ions; acidic if it contains a greater concentration of hydronium ions than hydroxide ions; and basic if it contains a lesser concentration of hydronium ions than hydroxide ions. A common means of expressing quantities that may span many orders of magnitude is to use a logarithmic scale. One such scale that is very popular for chemical concentrations and equilibrium constants is based on the p-function, defined as shown where “X” is the quantity of interest and “log” is the base-10 logarithm: pX = −log X

PDF page 777: As discussed earlier, hydronium and hydroxide ions are present both in pure water and in all aqueous solutions, and their concentrations are inversely proportional as determined by the ion product of water (Kw). The concentrations of these ions in a solution are often critical determinants of the solution’s properties and the chemical behaviors of its other solutes, and specific vocabulary has been developed to describe these concentrations in relative terms. A solution is neutral if it contains equal concentrations of hydronium and hydroxide ions; acidic if it contains a greater concentration of hydronium ions than hydroxide ions; and basic if it contains a lesser concentration of hydronium ions than hydroxide ions. A common means of expressing quantities that may span many orders of magnitude is to use a logarithmic scale. One such scale that is very popular for chemical concentrations and equilibrium constants is based on the p-function, defined as shown where “X” is the quantity of interest and “log” is the base-10 logarithm: pX = −log X

PDF page 777: As discussed earlier, hydronium and hydroxide ions are present both in pure water and in all aqueous solutions, and their concentrations are inversely proportional as determined by the ion product of water (Kw). The concentrations of these ions in a solution are often critical determinants of the solution’s properties and the chemical behaviors of its other solutes, and specific vocabulary has been developed to describe these concentrations in relative terms. A solution is neutral if it contains equal concentrations of hydronium and hydroxide ions; acidic if it contains a greater concentration of hydronium ions than hydroxide ions; and basic if it contains a lesser concentration of hydronium ions than hydroxide ions. A common means of expressing quantities that may span many orders of magnitude is to use a logarithmic scale. One such scale that is very popular for chemical concentrations and equilibrium constants is based on the p-function, defined as shown where “X” is the quantity of interest and “log” is the base-10 logarithm: pX = −log X

PDF page 778: + pH = −log[H O ] 3 Rearranging this equation to isolate the hydronium ion molarity yields the equivalent expression: −pH + [H O ] = 10 3 Likewise, the hydroxide ion molarity may be expressed as a p-function, or pOH: − pOH = −log[OH ] or −pOH − [OH ] = 10 Finally, the relation between these two ion concentration expressed as p-functions is easily derived from the Kw expression: + − Kw = [H O ][OH ] 3

PDF page 778: + pH = −log[H O ] 3 Rearranging this equation to isolate the hydronium ion molarity yields the equivalent expression: −pH + [H O ] = 10 3 Likewise, the hydroxide ion molarity may be expressed as a p-function, or pOH: − pOH = −log[OH ] or −pOH − [OH ] = 10 Finally, the relation between these two ion concentration expressed as p-functions is easily derived from the Kw expression: + − Kw = [H O ][OH ] 3

PDF page 778: + pH = −log[H O ] 3 Rearranging this equation to isolate the hydronium ion molarity yields the equivalent expression: −pH + [H O ] = 10 3 Likewise, the hydroxide ion molarity may be expressed as a p-function, or pOH: − pOH = −log[OH ] or −pOH − [OH ] = 10 Finally, the relation between these two ion concentration expressed as p-functions is easily derived from the Kw expression: + − Kw = [H O ][OH ] 3

PDF page 778: At 25 °C, the value of Kw is 1.0 × 10 , and so: 14.00 = pH + pOH

PDF page 778: pH = −log[H O ] = −log(1.0 × 10 ) = 7.00

PDF page 778: And so, at this temperature, acidic solutions are those with hydronium ion molarities greater than 1.0 × 10 M

PDF page 778: and hydroxide ion molarities less than 1.0 × 10 M (corresponding to pH values less than 7.00 and pOH values

PDF page 778: greater than 7.00). Basic solutions are those with hydronium ion molarities less than 1.0 × 10 M and hydroxide ion

PDF page 778: molarities greater than 1.0 × 10 M (corresponding to pH values greater than 7.00 and pOH values less than 7.00). Since the autoionization constant Kw is temperature dependent, these correlations between pH values and the acidic/ neutral/basic adjectives will be different at temperatures other than 25 °C. For example, the “Check Your Learning”