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Arlecino [84]
3 years ago
10

Calculate the molarity of 1.60L of a solution containing 1.55g of dissolved KBr

Chemistry
1 answer:
Olegator [25]3 years ago
7 0

Answer: the molarity is .00814

Explanation:the formula for molarity is moles over liters but we have grams so we do given over one so 1.55 over 1 multiplied by 1/119.0023 which is tht two atomc masses addes together then you get the moles and divde them by the liters to get the molarity hope this helps god bless

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Option D. 30 mL.

Explanation:

Step 1:

The balanced equation for the reaction. This is given below:

HNO3 + KOH —> KNO3 + H2O

From the balanced equation above,

The mole ratio of the acid, nA = 1

The mole ratio of the base, nB = 1

Step 2:

Data obtained from the question. This include the following:

Volume of base, KOH (Vb) =.?

Molarity of base, KOH (Mb) = 0.5M

Volume of acid, HNO3 (Va) = 10mL

Molarity of acid, HNO3 (Ma) = 1.5M

Step 3:

Determination of the volume of the base, KOH needed for the reaction. This can be obtained as follow:

MaVa / MbVb = nA/nB

1.5 x 10 / 0.5 x Vb = 1

Cross multiply

0.5 x Vb = 1.5 x 10

Divide both side by 0.5

Vb = (1.5 x 10) /0.5

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Therefore, the volume of the base, KOH needed for the reaction is 30mL.

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