All categories

2 years ago

How much of a 0.250 M lithium hydroxide is required to neutralize 20.0 mL of 0.345M chlorous acid?

Chemistry

1 answer:

Bumek [7]2 years ago

6 0

Answer:

27.6mL of LiOH 0.250M

Explanation:

The reaction of lithium hydroxide (LiOH) with chlorous acid (HClO₂) is:

LiOH + HClO₂ → LiClO₂ + H₂O

<em>That means, 1 mole of hydroxide reacts per mole of acid</em>

Moles of 20.0 mL = 0.0200L of 0.345M chlorous acid are:

0.0200L ₓ (0.345mol / L) = <em>6.90x10⁻³ moles of HClO₂</em>

To neutralize this acid, you need to add the same number of moles of LiOH, that is 6.90x10⁻³ moles. As the LiOH contains 0.250 moles / L:

6.90x10⁻³ moles ₓ (1L / 0.250mol) = 0.0276L of LiOH =

You might be interested in

Which best describes an element?

Aleonysh [2.5K]

I think the answer is a pure substance

6 0

2 years ago

Two charged particles repel each other with a force of F.

mihalych1998 [28]

Answer:

it would increase to twice what it was

3 0

2 years ago

Find the percentage composition of each element in the compound having 9.8 grams of nitrogen,0.7 grams of hydrogen and 33.6 gram

prisoha [69]

Answer: The percentage composition of nitrogen , hydrogen and oxygen is 22.2 % , 1.59 % and 76.2% respectively.

Explanation:

Percentage composition is defined as the ratio of mass of substance to the total mass in terms of percentage.

Percentage composition= $\frac{\text {mass of the element}}{\text {Total mass of the substance}}\times 100\%$

a) ${\text {percentage composition of nitrogen}}=\frac{\text {mass of nitrogen}}{\text {Total mass}}\times 100\%$

${\text {percentage composition of nitrogen}}=\frac{9.8g}{9.8+0.7+33.6}\times 100\%=22.2\%$

b) ${\text {percentage composition of hydrogen}}=\frac{\text {mass of hydrogen}}{\text {Total mass}}\times 100\%$

${\text {percentage composition of hydrogen}}=\frac{0.7}{9.8+0.7+33.6}\times 100\%=1.59\%$

c) ${\text {percentage composition of oxygen}}=\frac{\text {mass of oxygen}}{\text {Total mass}}\times 100\%$

${\text {percentage composition of oxygen}}=\frac{33.6}{9.8+0.7+33.6}\times 100\%=76.2\%$

The percentage composition of nitrogen , hydrogen and oxygen is 22.2 % , 1.59 % and 76.2% respectively.

4 0

2 years ago

How many particles are in a mole? 6.02 × 1023 23 × 106 602 billion 6.02 × 2310

Amanda [17]

Answer:

$1mole=6.02x10^{23} unit$ (Avogadro constant)

Explanation:

It is known by the name of mole (mol) to one of the fundamental physical magnitudes that contemplate the International System of Units. This unit is used to measure the quantity of all kinds of substances present in a given system.

The mole, experts say, reflects the amount of substance that has a specific number of entities of elementary character as atoms can be found in twelve grams of carbon-12. This means that the number of elementary units (as in the case of atoms, molecules or ions, for example) that are reflected in a mole of substance is a constant that has no direct relationship with the type of particle or material in question. This amount is known as Avogadro's number.

This constant, baptized in homage to the scientist of Italian origin Amedeo Avogadro (1776-1856), allows to count microscopic particles from macroscopic measurements (as it is the case of the mass).

6 0

3 years ago

Read 2 more answers

If 5 L of butane is reacted what volume of carbon dioxide is produced ILL GIVE BRAINLIEST

Len [333]

Answer: First, here is the balanced reaction: 2C4H10 + 13O2 ===> 8CO2 + 10H2O.

This says for every mole of butane burned 4 moles of CO2 are produced, in other words a 2:1 ratio.

Next, let's determine how many moles of butane are burned. This is obtained by

5.50 g / 58.1 g/mole = 0.0947 moles butane. As CO2 is produced in a 2:1 ratio, the # moles of CO2 produced is 2 x 0.0947 = 0.1894 moles CO2.

Now we need to figure out the volume. This depends on the temperature and pressure of the CO2 which is not given, so we will assume standard conditions: 273 K and 1 atmosphere.

We now use the ideal gas law PV = nRT, or V =nRT/P, where n is the # of moles of CO2, T the absolute temperature, R the gas constant (0.082 L-atm/mole degree), and P the pressure in atmospheres ( 1 atm).

V = 0.1894 x 0.082 x 273.0 / 1 = 4.24 Liters.

Explanation:

8 0

2 years ago