A 10.0 % (m/m) solution of potassium chloride, KCl dissolved in water has a density of 1.06 g/mL. What is the molar concentration of this aqueous solution? Molar Mass (KCl) = 74.55 g/mol

1,42M

Explanation:

Molar concentration is given in moles of solute per liter o solution. Assuming you have 100g of solution:

10g KCl × (1mol / 74,55g) = 0,134 moles of KCl

As you have 100g of solution:

100g × (1mL / 1,06g) × (1L / 1000mL) = 0,0943L

That means molar concentration is:

0,134 moles of KCl / 0,0943L = 1,42M

I hope it helps!

consider the reaction below.

 no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

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