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3 years ago

Si tomas 100ml de una solución de Nacl 4m y se disuelve en 200ml utilizando el mismo solvente ¿cuál será la nueva concentración?

Chemistry

1 answer:

g100num [7]3 years ago

3 0

Respuesta:

2 m

Explicación:

Paso 1: Información provista

Volumen inicial (V₁): 100 mL

Concentración inicial (C₁): 4 m

Volumen final (V₂): 200 mL

Concentración final (C₂): ?

Paso 2: Calcular la concentración de la solución final

Queremos perparar una concentración diluida a partir de una concentrada. Podemos calcular la concentración de la solución diluida usando la regla de dilución.

C₁ × V₁ = C₂ × V₂

C₂ = C₁ × V₁ / V₂

C₂ = 4 m × 100 mL / 200 mL = 2 m

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Archy [21]

Answer:

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Explanation:

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In this case, given the solubilization of cadmium (II) hydroxide:

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The solubility product can be set up as follows:

$Ksp=[Cd^{2+}][OH^-]^2$

Now, since we know the concentration of cadmium (II) ions at equilibrium and the mole ratio of these ions to the hydroxide ions is 1:2, we infer that the concentration of the latter at equilibrium is 3.5x10⁻⁵ M. In such a way, the resulting Ksp turns out to be:

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3 years ago

A 0.100 mile sample of gas is at a temperature of 85.0 degrees C and a volume of 3.47 L. What is the pressure of the gas( in mm

vladimir1956 [14]

Answer: 64.6 mmHg

Explanation:

Given that:

Volume of gas V = 3.47L

(since 1 liter = 1dm3

3.47L = 3.47dm3)

Temperature T = 85.0°C

Convert Celsius to Kelvin

(85.0°C + 273 = 358K)

Pressure P = ?

Number of moles of gas N = 0.100 mole

Note that Molar gas constant R is a constant with a value of 0.0082 ATM dm3 K-1 mol-1

Then, apply ideal gas equation

pV = nRT

p x 3.47dm3 = 0.10 x (0.0082 atm dm3 K-1 mol-1 x 358K)

p x 3.47dm3 = 0.29 atm dm3

p = (0.29 atm dm3 / 3.47 dm3)

p = 0.085 atm

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0.085atm = 0.085 x 760

= 64.6 mm Hg

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4 years ago

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trapecia [35]

Answer:

See explaination

Explanation:

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