Here, [OH-] = 10-7 M
pOH = -Log[OH-]
= -Log(10-7)
= 7
pH = 14 - pOH
= 14 - 7
= 7
Therefore, the pH of a solution that has a hydroxide ion concentration of 1.0*10-7 M = 7
Part (ii): The pOH of 0.1 M solution of NaOH = -Log(0.1) = 1
i.e. pH = 14 - 1 = 13
0.10 m soultions of sodium hydroxide 7.48 Part A What is the pH of a solution...
1)What is the pH of an aqueous solution of 5.51×10-2 M sodium hydroxide? pH =_____ 2)The pH of an aqueous solution at 25°C was found to be 7.30. The pOH of this solution is ______. The hydronium ion concentration is ______ M. The hydroxide ion concentration is ______ M. 3)The hydronium ion concentration in an aqueous solution at 25°C is 3.1×10-2M. The hydroxide ion concentration is ____M. The pH of this solution is ____. The pOH is _____ .
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Question 4 of 65 > What is the pH of an aqueous solution with a hydroxide ion concentration of 3.20 x 10-4 M? O 14.5 O 3.49 10.5 0 -0.505
What is the hydroxide-ion concentration of a 0.250 M sodium oxalate (Na2C2O4) solution?For oxalic acid (H2C2O4), Ka1 = 5.6×10–2 and Ka2 = 5.1×10–5.
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