I'm a little confused on how to do the calculations. How do I do the calculations for this? Specifically the first or second calculation portion.  The theoretical number of moles of OH– needed to change the pH by one unit (refer to Appendix 7 for a sample calculation and explanation as to why moles  are being used) pHi + ∆pH = pKa + log ( mol A− + mol OH− mol HA − mol OH−

Determine the [OH−], pH, and pOH of a solution with a [H+] 7.7×10^−11 M at 25 °C [OH−]=     pH=     pOH=     Determine the [H+], pH, and pOH of a solution with an [OH−] of 7.0×10−8 Mat 25 °C   H+]=     pH=     pOH=     Determine the [H+], [OH−], and pOH of a solution with a pH of 11.75 at 25 °C   [H+]=     [OH−]=     pOH=     Determine the [H+], [OH−], and pH of a solution with a pOH of 7.38 at 25 °C   [H+]=     [OH−]=     pH=

What is the pH of a solution of 1.0 × 10-9 M NaOH (include 1 digit after the decimal in your answer)?

Determine the [OH−], pH, and pOH of a solution with a [H+]of 5.7×10−9 M at 25 °C. [OH−]=     pH=     pOH=     Determine the [H+] , pH, and pOH of a solution with an [OH−] of 5.1×10−9 M at 25 °C. [H+]=   MM pH=     pOH=     Determine the [H+] , [OH−] , and pOH of a solution with a pH of 3.063.06 at 25 °C. [H+]=     [OH−]=     pOH=     Determine the [H+][H+] , [OH−][OH−] , and pH of a solution with a pOH of 5.525.52 at 25 °C. [H+]=     [OH−]=     pH=