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2 years ago

Salts and acids are examples of inorganic compounds called _____, which dissociate in water to release ions.

Chemistry

2 answers:

g100num [7]2 years ago

8 0

Salts and acids are examples of inorganic compounds called Electrolytes which dissociate in water to release ions.

<h2>Further Explanation: </h2><h3>A compound </h3>

A compound is a substances that contains two or more different atoms that are bonded together.
When the atoms are similar the substance is known as a molecule, therefore not all molecules are compounds.

<h3>Electrolytes</h3>

Electrolytes are substances that are either in molten or aqueous form that discharged by passing electric current through them. They dissociate into ions while in molten or solution form.
These compounds are made of mobile ions which are responsible for the conduction of electricity.
Examples includes, soluble salts, ionic compounds, acids, and bases etc.

A salt is a substance that is formed when an acid reacts with a base or when the hydrogen part of acid is replaced by metal ion or an ammonium ion.

<h3>Ionic compounds </h3>

Ionic compounds are compounds that contain ions. They are as a result of ionic bonding between a metal atom and a non-metal atom.
During ionic bonding formation the metallic atom looses electrons while the non-metallic atom gains electrons.
Ionic compounds contains both negatively charged ion(anion) and positively charged ion (cation).
Examples of ionic compounds, NaCl, LiF, KCl, Cs2S, KBr, PbS etc.
Most ionic compounds may act as electrolytes.

Keywords: Compound, electrolytes, salts, ionic compounds, soluble acids, bases.

<h3>Learn more about: </h3>

Compound: brainly.com/question/10052458
Electrolytes: brainly.com/question/4053091
Electrolysis: brainly.com/question/11868966
Ionic compounds: brainly.com/question/10052458

Level: High school

Subject: Chemistry

Topic: Electrolysis

Sub-topic: Electrolytes.

Blizzard [7]2 years ago

4 0

Answer:

Salts and acids are examples of inorganic compounds called <u><em>electrolytes</em></u>.

Explanation:

Electrolytes are the substances which dissociates into ions when dissolved in water and due to this they are able to conduct electric current through them. These compounds in solid form does not conduct electricity due to the absence of free ions.

For example: Sodium chloride , sulfuric acid etc.

$NaCl(aq)\righarrow = Na^+(aq)+Cl^-(aq)$

$H_2SO_4(aq)\rightarrow SO_4^{2-}(aq)+2H^+(aq)$

You might be interested in

If 4.59 g of potassium reacts with 3.6 g of sulfur according to the following reaction, how many grams of potassium sulfide can

EleoNora [17]

First convert the amount of grams you have of each substance to moles. Find your limiting reactant by calculating how many grams are needed to complete this reaction. If done correctly, you would see that we need .226 moles of Potassium to complete this reaction. However, we only have .118 moles of Potassium, so K must be our limiting reactant. Then use the moles of K to find out how many moles of K^2S are made. Then convert the amount of moles of K^2S to grams and you should get 10.3 g K^2S

8 0

2 years ago

SnO2 is reduced by carbon according to this reaction: SnO2 + C ???? Sn + CO2. How many liters of CO2 are produced if 300.0 grams

andrew-mc [135]

Explanation:

The given reaction is as follows.

$SnO_{2} + C \rightarrow Sn + O_{2}$

a). Molar mass of $SnO_{2}$ is [(mass of Sn) + (2 × mass of O)].

Therefore, molar mass of $SnO_{2}$ = (118.7 + 2 × 16) g/mol = 150.7 g/mol

Since, it is known that number of moles equal mass divided by molar mass. So, moles of Sn will be calculated as follows.

No. of moles = $\frac{mass}{molar mass of SnO_{2}}$

= $\frac{300 g}{150.7 g/mol}$

= 2.53 mol

As it is given that 1 mole of $SnO_{2}$ produces 1 moles of Sn and 1 moles of $CO_{2}$ . Hence, 2.53 moles of $SnO_{2}$ will also produce 2.53 moles of Sn and 2.53 moles of $CO_{2}$ .

Volume of 1 mole of $CO_{2}$ at STP is 22.4 L. Therefore, volume of 2.53 moles of $CO_{2}$ will be calculated as follows.

2.53 × 22.5 L = 56.67 L

Hence, 56.67 L of $CO_{2}$ are produced if 300.0 grams of tin are produced at STP.

b). Mass of tin is given as 1800.0 g. So, number of moles will be calculated as follows.

No. of moles = $\frac{mass}{molar mass of tin}$

= $\frac{1800.0 g}{118.7 g/mol}$

= 15.2 moles

As 15.2 moles of $SnO_{2}$ produces 15.2 moles of Sn. Therefore, weight of $SnO_{2}$ will be calculated as follows.

Mass = no. of moles × molar mass of $SnO_{2}$

= 15.2 moles × 150.7 g/mol

= 2290.64 g

Hence, 2290.64 grams of $SnO_{2}$ are required to produce 1800.0 grams of tin.

c). Mass of carbon given is 100.0 grams.

No. of moles = $\frac{mass}{molar mass of carbon}$

= $\frac{100 g}{12 g/mol}$

= 8.33 moles

As, 1 mole of carbon is produced by 1 mole of tin. So, 8.33 mole of carbon will be produced by 8.33 moles of tin.

Therefore, calculate mass of tin produced as follows.

Mass = no. of moles × molar mass of Sn

= 8.33 moles × 118.7 g/mol

= 988.8 g

Hence, 988.8 grams of tin will be produced per 100 grams of carbon used.

8 0

2 years ago

A gas in a rigid container at 25°C has a pressure of 0.96 atm. A change in temperature causes the pressure to increase to 1.25 a

m_a_m_a [10]

Gay-Lussacs law states that pressure of a gas is directly proportional to temperature when the volume is kept constant

P / T = k

where P - pressure , T - temperature in kelvin and k - constant

$\frac{P1}{T1} = \frac{P2}{T2}$

where parameters for the first instance are on the left side of the equation and parameters for the second instance are on the right side of the equation

T1 - 25 °C + 273 = 298 K

substituting the values in the equation

$\frac{0.96 atm}{298 K}= \frac{1.25 atm}{T2}$