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Irina18 [472]
2 years ago
11

HELP ASAP!!!!!!!!!!! * worth 35 points + brainliest *

Chemistry
2 answers:
gizmo_the_mogwai [7]2 years ago
7 0

Explanation:

According to Arrhenius concept:

A base is defined as a substance which donates hydroxide ions (OH^-).When they are dissolved water it gives out hydroxide ions.

BOH(aq)\rightarrow B^+(aq)+OH^-(aq)

For example sodium hydroxide pellets when dissolved in water gives sodium ions and hydroxide ions.

NaOH\rightarrow Na^+(aq)+OH^-(aq)

Properties of Arrhenius bases:

  • They slippery in touch
  • They are bitter in taste if ingested.
  • They turn litmus paper blue.
  • They react with acid to undergo neutralization reaction in which water and salt is formed.
  • They pH value is always greater than  7.

An acid is defined as a substance which donates hydronium ions (H_3O^+) .When they are dissolved water it gives out hydronium ion.

AH(aq)\rightarrow A^-(aq)+H_3O^+(aq)

Musya8 [376]2 years ago
6 0

Answer:

In chemistry, a base is a substance that is slippery to the touch and has a pH greater than 7. If you were to eat a base (which you should not do) it would have bitter to the taste. A perfect example of a base is soap - when you touch soap, it feels slippery. Have you ever accidentally tasted soap? You may notice that it has a bitter taste.

These are some physical characteristics of bases, but what about the theory behind the behavior of bases when they are in a solution? There are many theories from different scientists that describe a base. One Swedish scientist, named Svante Arrhenius, came up with the theory of a base in 1884. Svante Arrhenius' definition of a base is what we now refer to as an Arrhenius base.

An Arrhenius base is a substance that, when dissolved in an aqueous solution, increases the concentration of hydroxide, or OH-, ions in the solution. An aqueous solution is a solution that has water present in it. Let's imagine dissolving a basic substance in water. According to Svante Arrhenius, when a base dissolves in an aqueous solution, it dissociates into ions and releases hydroxide ions.

NaOH dissociates into sodium, Na+, and hydroxide, OH-, ions. Because the hydroxide ions are released in the aqueous solution, the hydroxide concentration increases; therefore, NaOH is an Arrhenius base.

Sodium hydroxide, when dissolved in an aqueous solution, releases hydroxide ions in the solution.

The water above the arrow means that the NaOH is added or combined with water and dissociates into sodium, a positive cation, and one or more negative hydroxide anions.

Explanation:

Hope this helps

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Nuetrik [128]

Answer:

a. The maximum volume of 0.143 M HCl required is 154.4 mL.

b. The maximum volume of 0.143 M HCl required is 135.7 mL.

Explanation:

a.

Al(OH)_3+3HCl\rightarrow AlCl_3+3H_2O

Mass of aluminum hydroxide = 350 mg =  0.350 g ( 1mg = 0.001 g)

Moles of aluminum hydroxide = \frac{0.350 g}{78 g/mol}=0.004487 mol

According to reaction ,3 moles of HCl neutralize 1 mole of aluminum hydroxide.Then 0.004487 mole of aluminum hydroxide will be neutralize by :

\frac{3}{1}\times 0.004487 mol=0.01346 mol of HCl.

Mg(OH)_2+2HCl\rightarrow MgCL_2+2H_2O

Mass of magnesium hydroxide = 250 mg =  0.250 g ( 1mg = 0.001 g)

Moles of magnesium hydroxide = \frac{0.250 g}{58 g/mol}=0.004310 mol

According to reaction ,2 moles of HCl neutralize 1 mole of magnesium hydroxide.Then 0.004310  mole of magnesium hydroxide will be neutralize by :

\frac{2}{1}\times 0.004310 mol=0.008621 mol of HCl.

Total moles of HCl required to neutralize both :

0.01346 mol + 0.008621 mol = 0.02208 mol

Molarity of the HCL solution = 0.143 M

Volume of the solution = V

Molarity=\frac{\text{Total moles of HCl}{\text{Volume in Liter}}

V=\frac{0.02208 mol}{0.143 M}=0.1544 L

1 L = 1000 mL

0.1544 L = 154.4 mL

The maximum volume of 0.143 M HCl required is 154.4 mL.

b.

CaCO_3+2HCl\rightarrow CaCl_2+H_2O+CO_2

Mass of calcium carbonate = 970mg =  0.970 g ( 1mg = 0.001 g)

Moles of calcium carbonate = \frac{0.970 g}{100 g/mol}=0.00970 mol

According to reaction ,2 moles of HCl neutralize 1 mole of calcium carbonate.Then 0.00970 mole of calcium carbonate will be neutralize by :

\frac{2}{1}\times 0.00970 mol=0.0194 mol of HCl.

Total moles of HCl required to neutralize calcium carbonate : 0.0194 mol

Molarity of the HCL solution = 0.143 M

Volume of the solution = V

Molarity=\frac{\text{Total moles of HCl}}{\text{Volume in Liter}}

V=\frac{0.0194 mol}{0.143 M}=0.1357 L

1 L = 1000 mL

0.1357 L = 135.7 mL

The maximum volume of 0.143 M HCl required is 135.7 mL.

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