Question

The problem is for part (c) below.Thank you.
Calculate [H⁺] for each of the following solutions,and indicate whether the solution is acidic, basic, orneutral.(a) [OH ^-] = 0.00041 M
M ---Select---acidicbasicneutral

(b) [OH ^-] = 2.5 10^-9 M
M ---Select---acidicbasicneutral

(c) a solution in which [OH ^-] is 100 times greater than[H⁺]

Your answer differs from the correct answerby orders of magnitude. M ---Select---acidicbasicneutral

Answer 1

If pH is 1-6.9 then it is acidIf pH is 7.1 - 14 then it is Basea)pOH = -log[OH]=-log(0.00041)=3.38pH = 14-pOH= 14-3.38= 10.612So it is Baseb) pOH = -log(2.5*10^-9)=8.602pH = 14-pOH= 14-8.602= 5.3Hence it is acidicc) we know that[H⁺][OH^-] =10^-14here [OH^-] is 100 times getter then[H⁺]so 100[H⁺][H⁺] =10^-14∴[H⁺] =10^-8Total concentration of [H⁺] in solution[H⁺] =10^-7 + 10^-8= 10^-7 (1+0.1)=10^-7 (1.1)pH = -log[H⁺]=-log10^-7 (1.1)= 7-log(1.1)= 7-0.0413= 6.95Hence it is acidic