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3 years ago

9. Calculate the percentage composition of silver sulfate, Ag2SO4.

Chemistry

1 answer:

riadik2000 [5.3K]3 years ago

7 0

Answer:

69% Ag, 10.5% S, 20.5% O.

Explanation:

Ag₂SO₄ → Molar mass = 311.8 g/mol

2 mol of Ag → 107.87g/m . 2m = 215.74 g

1 mol of S → 32.06g/m . 1m = 32.06 g

4 mol of O → 16g/m .4m = 64 g

Percentage composition will be:

(Mass of Ag/ Total mass) . 100

(215.74 g / 311.8 g) . 100 = 69 %

(Mass of S/ Total mass) . 100

(32.06 g / 311.8 g) .100 = 10.5%

(Mass of O/ Total mass) . 100

(64 g / 311.8 g) . 100 = 20.5 %

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3 years ago

Please Help!!!!!!!

hichkok12 [17]

3,1,3,1

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Reaction equation:

HBr + Al(OH)₃ ⇒ H₂O + AlBr₃

To balance an equation we make sure that the same number of atoms appears on both sides of the expression.

HBr + Al(OH)₃ ⇒ H₂O + AlBr₃

Let us a simple mathematical method to solve this problem

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a, b , c and d are the coefficients that will make the equation balanced;

Conserving H; a + 3b = 2c

Br; a = 3d

Al; b = d

O; 3b = c

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d = $\frac{1}{3}$

b = $\frac{1}{3}$

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3 years ago

Which one of the following statements best describes a solution with a pH of 3?

zalisa [80]

Statement D is the correct option as the solution will have pH of 3. It has an H3O+ ion concentration of 1 × $10^{-3}$ mol/L and is acidic.

Explanation:

It is given in question that solution must have pH of 3. The value if being less than 7 shows that solution is acidic. The pH value of 3 indicates that given solution is highly acidic and has strong acid. Strong acid gets fully dissociated into $H_{3}$ $O^{+}$ ions.

pH of the solution is calculated as:

pH = -log10[ $H_{3}$ $O^{+}$ ]

the concentration or molarity of the hydronium ion is given as moles/litre

concentration of hydronium ion in the solution is 1 X $10^{-3}$ moles/litre

putting the values in the equation:

pH = - log10( 1 X $10^{-3}$ )

pH = 3 (acidic)

Thus it can be concluded that D option is the right answer.

6 0

4 years ago