A student adds 5.85 gm of NaCl to 1 litre of water (the pH of which was measured to be 7.0) in a flask (X)
to make a 0.1 M solution. He transfers 500 ml into another flask (Y). He covers the flask (Y) with tissue
paper and the original flask (X) with a watch glass and goes to watch a movie. When he returns to the lab
the next morning, he checks the pH of both the solutions using a perfectly calibrated pH meter. Which of
the following is correct?
A) X has pH =7 and Y has pH > 7
B) X has pH < 7 and Y has pH = 7
C) X has pH = 7 and Y has pH < 7
D) Both X and Y have pH = 7
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Answer:
12th
Chemistry
Solutions
Expressing Concentration of Solutions
(a) 5.85 g of NaCl is disso...
CHEMISTRY
(a) 5.85 g of NaCl is dissolved in 200 mL of water. What will be the molarity of this solution?
(b) Calculate the molarity of the solution obtained by dissolving 20.6 g NaBr in 500 mL of water.
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ANSWER
Mole =
molecular weight
weight
Molecular weight of NaCl is 58.5
molarity of NaCl =
volume in L
mol
=
58.5×0.2
5.85
= 0.5M
Molecular weight of NaBr is 103.
molarity of NaBr =
volume in L
mol
=
103×0.5
20.6
= 0.4M
Hence, option C is correct.
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