Cuantos miles de sulfato de calcio están en 60 gramos de sustancia

A chemist needs to determine the concentration of a sulfuric acid solution by titration with a standard sodium hydroxide solutio

Zigmanuir [339]

<u>Answer:</u> The concentration of original sulfuric acid solution is 1.62 M

<u>Explanation:</u>

Let the original concentration of sulfuric acid be 'x' M

To calculate the molarity of the diluted solution, we use the equation:

$M_1V_1=M_2V_2$

where,

$M_1\text{ and }V_1$ are the molarity and volume of the concentrated sulfuric acid solution

$M_2\text{ and }V_2$ are the molarity and volume of diluted sulfuric acid solution

We are given:

$M_1=xM\\V_1=25.00mL\\M_2=?M\\V_2=250.0mL$

Putting values in above equation, we get:

$x\times 25.00=M_2\times 250.0\\\\M_2=\frac{x\times 25.0}{250}=\frac{x}{10}$

Now, to calculate the concentration of acid, we use the equation given by neutralization reaction:

$n_1M_1V_1=n_2M_2V_2$

where,

$n_1,M_1\text{ and }V_1$ are the n-factor, molarity and volume of acid which is $H_2SO_4$

$n_2,M_2\text{ and }V_2$ are the n-factor, molarity and volume of base which is NaOH.

We are given:

$n_1=2\\M_1=\frac{x}{10}M\\V_1=10.00mL\\n_2=1\\M_2=0.1790M\\V_2=18.07mL$

Putting values in above equation, we get:

$2\times \frac{x}{10}\times 10.00=1\times 0.1790\times 18.07\\\\x=\frac{1\times 0.1790\times 18.07\times 10}{2\times 10.00}=1.62M$

Hence, the concentration of original sulfuric acid solution is 1.62 M

5 0

4 years ago

Read this sentence from Chapter One of Jack London’s The Call of the Wild.

xenn [34]

Answer:

b)

Explanation:

It shows the natrual proggresion of a story and helps blend the narrtive together.

4 0

3 years ago

Read 2 more answers

Based on position in the periodic table and electron configuration, arrange these elements in order of decreasing Ei1.

irakobra [83]

Answer:

Rb<K<Ga<As<Se<S

Explanation:

We must remember that first ionization energy decreases down the group and increases across the period.

First ionization energy decreases down the group because of the addition of more shells which increases the distance between the nucleus and the outermost electron. Hence, Rb has a lower ionization energy that K.

Across the period, increase in the size of the nuclear charge causes the pull of the nucleus on the outermost electrons to increase thereby increasing the ionization energy. Hence ionization energy increases across the period. For this reason, the ionization energy of Ga<As<Se as shown.

4 0

4 years ago

What is the pH of a solution in which [OH-] = 1.0 x 10-2 M

Degger [83]

Answer:

12

Explanation:

pOH = -log(1.0 x 10^-2) = 2

pH = 14 - pOH

pH = 14 - 2 = 12

7 0

3 years ago

An oily liquid with a cheesy, waxy odor like that of goats or other barnyard animals is caproic acid, a compound containing carb

Zinaida [17]

The empirical formula for the caproic acid, given the combustion analysis data is C₃H₆O

We'll begin bey obtaining the mass of carbon, hydrogen and oxygen in the compound. This is illustrated below:

How to determine the mass of C

Mass of CO₂ = 9.78 g
Molar mass of CO₂ = 44 g/mol
Molar of C = 12 g/mol
Mass of C =?

Mass of C = (12 / 44) × 9.78

Mass of C = 2.67 g

How to determine the mass of H

Mass of H₂O = 20.99 g
Molar mass of H₂O = 18 g/mol
Molar of H = 2 × 1 = 2 g/mol
Mass of H =?

Mass of H = (2 / 18) × 4

Mass of H = 0.44 g

How to determine the mass of O

Mass of compound = 4.30 g
Mass of C = 2.67 g
Mass of H = 0.44 g
Mass of O =?

Mass of O = (mass of compound) – (mass of C + mass of H)

Mass of O = 4.30 – (2.67 + 0.44)

Mass of O = 1.19 g

<h3>How to determine the empirical formula </h3>

The empirical formula of the compound can be obtained as follow:

C = 2.67 g
H = 0.44 g
O = 1.19 g
Empirical formula =?

Divide by their molar mass

C = 2.67 / 12 = 0.2225

H = 0.44 / 1 = 0.44

O = 1.19 / 16 = 0.074

Divide by the smallest

C = 0.2225 / 0.074 = 3

H = 0.44 / 0.0744 = 6

O = 0.074 / 0.074 = 1

Thus, the empirical formula of the compound is C₃H₆O

Learn more about empirical formula:

brainly.com/question/9459553

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6 0

2 years ago