Asked by johnX
A)Whats the pH of Distilled water.(is it really 7 or can be 6).
B)Also whats the pH of (4o ml DI water +1.0 ml of 6.0 M HCl)?
C)and also pH of (4o ml DI water +1.0 ml of 6.0 M NaOH)?
B)Also whats the pH of (4o ml DI water +1.0 ml of 6.0 M HCl)?
C)and also pH of (4o ml DI water +1.0 ml of 6.0 M NaOH)?
Answers
Answered by
DrBob222
A). The pH of PURE water is 7.0. Distilled water CAN be less than 7.0 if it has absorbed some CO2 from the air.
B) The 6.0 M HCl has been diluted 1 mL to 41 mL; therefore, molarity of HCl is
6.0 x (1/41) = ??.
HCl is a strong electrolyte and ionizes 100%; therefore, the H^+ is the same as the molarity.
pH = - log(H^+)
C)This is done the same way as (b) except you have NaOH instead of HCl. Therefore, the diluted molarity of the NaOH = (OH^-).
pOH = - log (OH^-)
and pH + pOH = 14
B) The 6.0 M HCl has been diluted 1 mL to 41 mL; therefore, molarity of HCl is
6.0 x (1/41) = ??.
HCl is a strong electrolyte and ionizes 100%; therefore, the H^+ is the same as the molarity.
pH = - log(H^+)
C)This is done the same way as (b) except you have NaOH instead of HCl. Therefore, the diluted molarity of the NaOH = (OH^-).
pOH = - log (OH^-)
and pH + pOH = 14
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