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2 years ago

HELP PLEASE!!!!!!!!

Chemistry

1 answer:

Ray Of Light [21]2 years ago

6 0

Reactant is the left side. 4+3=7

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A chemist dissolves 797. mg of pure barium hydroxide in enough water to make up 60. mL of solution. Calculate the pH of the solu

topjm [15]

Answer:

13.20

Explanation:

Step 1: Calculate the moles of Ba(OH)₂

The molar mass of Ba(OH)₂ is 171.34 g/mol.

0.797 g × 1 mol/171.34 g = 4.65 × 10⁻³ mol

Step 2: Calculate the molar concentration of Ba(OH)₂

Molarity is equal to the moles of solute divided by the liters of solution.

[Ba(OH)₂] = 4.65 × 10⁻³ mol/60 × 10⁻³ L = 0.078 M

Step 3: Calculate [OH⁻]

Ba(OH)₂ is a strong base according to the following equation.

Ba(OH)₂ ⇒ Ba²⁺ + 2 OH⁻

The concentration of OH⁻ is 2/1 × 0.078 M = 0.16 M

Step 4: Calculate the pOH

pOH = -log OH⁻ = -log 0.16 = 0.80

Step 5: Calculate the pH

We will use the following expression.

pH + pOH = 14

pH = 14 - 0.80 = 13.20

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2 years ago

Pls help me will mark Brianliest!!! I know the answer choice is a bit cut off. Topic is chem equilibrium

Svetlanka [38]

Answer:

See notes on LeChatlier's Principle I gave you yesterday.

Explanation:

Remember chemical see-saw => Removing Fe⁺³ makes the reactant side of the see-saw lighter causing the balance to tilt right then shift left to establish a new equilibrium with new concentration values. Such would result in a decrease in FeSCN⁺² concentration and increases in Fe⁺³ and SCN⁻ concentrations to replace the original amount of ppt'd Fe⁺³. => Answer Choice 'B' ... Also, see attached => Concentration effects on stability of chemical equilibrium .

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2 years ago

CHM 17 Practice Final Exam

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Answer:

moneyyyyyyyyfght

Explanation:

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