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3 years ago

Pre-laboratory Assignment For full credit, show the details of each calculation below. Use more paper if needed.

Chemistry

1 answer:

Triss [41]3 years ago

6 0

Answer:

1. Answers are in the question.

2. a. 61.8 w/w%

b. 61.8g solute per 100g of solvent

Explanation:

a. Solvent is a substance (Usually liquid) that is able to dissolve a substance (Solute).

b. Solution is the mixture of a solute and a solvent.

c. A saturated solution is defined as the solution that contains the maximum amount of solute that a solvent can dissolve.

2. Mass percent is:

Mass solute / Mass solution * 100

17.5g / 28.3g * 100 =

a. 61.8 w/w%

Solubility is the concentration of a saturated solution. 100g of solvent will dissolve:

17.5g solute * (100g / 28.3g) = 61.8g of solute can be dissolved per 100g of solute.

Solubility is:

b. 61.8g solute per 100g of solvent

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What is the Ksp of nickel(II) sulfide if the equilibrium concentrations of Ni2+ and S2− in a saturated solution of NiS are each

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As a chemist for an agricultural products company, you have just developed a new herbicide,"Herbigon," that you think has the po

Ganezh [65]

Answer:

pH = 2.03

Explanation:

The pH can be calculated using the following equation:

$pH = -log [H_{3}O^{+}]$ (1)

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$K_{sp} = [CH_{3}COO^{-}][X^{+}]$

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By entering the values of [CH₃COO⁻] and Ka, into equation (2) we can calculate [H₃O⁺]:

$[H_{3}O^{+}] = \frac{1.74 \cdot 10^{-5}*[1.00]}{[1.88 \cdot 10^{-3}]} = 9.26 \cdot 10^{-3} M$

Hence, the pH is:

$pH = -log [H_{3}O^{+}] = -log [9.26 \cdot 10^{-3}] = 2.03$

Therefore, the pH must be 2.03 to yield a solution in which the concentration of X⁺ is 5.00x10⁻³M.

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