You have an aqueous solution with a ph of 8.0. You add sodium chloride to a concentration of 1 gram per 100 milliliters. What ha

Let's assume that the compound formula is as follows: Experiment 1: 1.00 g of the compound yields 1.95 g of AgCl. The molar mass of AgCl is 143.32 g/mol. Thus, the moles of AgCl for 1.95g are: The moles of Cl also equal 0.0136, considering that 1 mole of AgCl corresponds to 1 mole of Cl. Experiment 2: 1.00 g of the compound results in 0.900 g of CO2 and 0.735 g of H2O. The molar mass of CO2 is 44 g/mol, and for H2O, it's 18 g/mol. Therefore, the moles of C come to 0.0205 and the moles of H stand at 0.0816 (which is 2 times the moles of H2O). Now, from the provided details, it's derived that in 1.00 g of the compound, there are 0.0136 moles of Cl, 0.0205 moles of C, and 0.0816 moles of H. In terms of mass: Mass of Cl = 0.0136 * 35.5 = 0.4828 g. Mass of C = 0.0205 * 12 = 0.246 g. Mass of H = 0.0816 * 1 = 0.0816 g. Total mass = 0.4828 + 0.246 + 0.0816 + mass of N. Given that 1.00 = 0.8104 + Mass of N, it follows that Mass of N = 0.1896. Thus, upon dividing all moles by the smallest value, we find Cl = 0.0136 / 0.0135 = 1.0007; C = 0.0205 / 0.0135 = 1.52; H = 0.0816 / 0.0135 = 6.04; N = 0.0135 / 0.0135 = 1. Multiplying by 2 allows us to reach integer values: Cl = 2, C = 3, H = 12, N = 2.

Hi, Due to calcium hydroxide being a strong base, its full dissociation will yield both calcium and hydroxyl ions: Thus, the concentration of hydroxyl ions mirrors that of the calcium hydroxide, allowing for the calculation of pOH as demonstrated below: Now, pH relates to pOH as: Consequently, the final pH is achieved. Best regards.

To start, consult the periodic table to pinpoint the element with an average atomic mass of 24.3. The amu is simply the number listed under the element, leading us to conclude that Mg is the answer.

Answer:

Step 1:

N

H

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3

C

H

2

C

H

2

N

H

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3

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q

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K

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2

Step 2:

N

H

2

C

H

2

C

H

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N

H

+

3

(

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K

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B.

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Acid-

Respuesta:

737.52 mL de agua

Justificación:

En este escenario, es necesario aplicar la fórmula de molaridad de una solución, que es:

M = moles / V

Donde:

V: Volumen de la solución.

Ya que deseamos determinar la cantidad de agua, en otras palabras, buscamos el volumen del solvente que se utilizó para crear los 800 mL de la disolución.

Una disolución se compone de un soluto y un solvente. El soluto que tenemos es nitrato de plata. Utilizando la fórmula mencionada, calculamos los moles de soluto y luego su masa. Tras eso, calculamos el volumen a partir de la densidad y, al final, determinamos la cantidad de solvente de esta manera:

V ste = Vsol - Vsto

Primero, vamos a calcular los moles de soluto:

moles = M * V

moles = 2 * 0.800 = 1.6 moles

Con este número de moles, obtenemos la masa utilizando el peso molecular que es 169.87 g/mol:

m = moles * PM

m = 1.6 * 169.87 = 271.792 g

Usando el valor de densidad, procederemos a calcular el volumen de soluto utilizado:

d = m/V

V = m/d

V = 271.792 / 4.35

V = 62.48 mL

Por último, la cantidad de agua requerida es:

V agua = 800 - 62.48

V agua = 737.52 mL