Question 10 2 pts
(2 points) What is the molarity of a solution when 25.0 mL of 0.500 M NaCl is diluted to 150.0 mL?
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M₂  = 0.08 M

Explanation:

Given data:

Initial volume = 25.0 mL

Initial molarity = 0.500 M

Final volume = 150.0 mL

Final molarity = ?

Solution:

Formula:

M₁V₁          =     M₂V₂

0.500 M × 25.0 mL = M₂ ×  150.0 mL

M₂  = 0.500 M × 25.0 mL /   150.0 mL

M₂  = 12.5 M.mL /150.0 mL

M₂  = 0.08 M

when [oh-] is 10-5  m, and [h3o+] is 10-9  m, the poh is 5 and ph is 9. again in both cases the sum of ph and poh is 14. however, the hydrogen ion concentration is not always going to be equal to exactly 1 x 10 raised to a negative number. for example, we skipped over the value of 2.0 x 10-7.