All categories

3 years ago

Acids increase the concentration of __________ in a solution

Chemistry

2 answers:

Rufina [12.5K]3 years ago

3 0

A. hydroxide is the answer

Kaylis [27]3 years ago

3 0

Acids increase the concentration of A. Hydroxide

You might be interested in

Is cinnamon ionic or covalent ?

myrzilka [38]

it is covalent because it does not dissolve in water

5 0

3 years ago

Read 2 more answers

During science lab, Carl notices that when he adds water to his solid sample of anhydrous copper

Bond [772]

Answer:

The dissociation of copper sulfate into ions is an exothermic chemical reaction that releases heat into the surroundings.

Explanation:

Some of the potential energy stored in the solid sample of anhydrous copper sulfate is released as heat as the sample dissolves and dissociates into ions in the water. This is due to the large lattice energy of the crystalline copper sulfate.

hope this helps

4 0

3 years ago

Why is urbanization contributing to pollution? People in urban areas strip the soil of nutrients and make it difficult to grow c

slavikrds [6]

We have to know how urbanization causes pollution.

The reason is: People in urban areas consume more energy, food, and water.

Urbanisation is one of the major problem towards pollution. The smoke from automobiles, factories and power generators make air unhealthy. Also chemical spills and other toxic gases contaminate in air.

The mixing of toxins in the soil is polluting soil which disturbs eco-system.

The high density population in urban area consume more energy , food and water which causes pollution.

7 0

3 years ago

Read 2 more answers

A buffer solution is made that is 0.347 M in H2C2O4 and 0.347 M KHC2O4.

irga5000 [103]

Answer:

1. pH = 1.23.

2. $H_2C_2O_4(aq) +OH^-(aq)\rightarrow HC_2O_4^-(aq)+H_2O(l)$

Explanation:

Hello!

1. In this case, for the ionization of H2C2O4, we can write:

$H_2C_2O_4\rightleftharpoons HC_2O_4^-+H^+$

It means, that if it is forming a buffer solution with its conjugate base in the form of KHC2O4, we can compute the pH based on the Henderson-Hasselbach equation:

$pH=pKa+log(\frac{[base]}{[acid]} )$

Whereas the pKa is:

$pKa=-log(Ka)=-log(5.90x10^{-2})=1.23$

The concentration of the base is 0.347 M and the concentration of the acid is 0.347 M as well, as seen on the statement; thus, the pH is:

$pH=1.23+log(\frac{0.347M}{0.347M} )\\\\pH=1.23+0\\\\pH=1.23$

2. Now, since the addition of KOH directly consumes 0.070 moles of acid, we can compute the remaining moles as follows:

$n_{acid}=0.347mol/L*1.00L=0.347mol\\\\n_{acid}^{remaining}=0.347mol-0.070mol=0.277mol$

It means that the acid remains in excess yet more base is yielded due to the effect of the OH ions provided by the KOH; therefore, the undergone chemical reaction is:

$H_2C_2O_4(aq) +OH^-(aq)\rightarrow HC_2O_4^-(aq)+H_2O(l)$

Which is also shown in net ionic notation.

Best regards!

4 0

3 years ago

If 45 mL of water are added to 250 mL of a 0.75 M K2SO4 solution, what will the molarity of the diluted solution be?

krok68 [10]

Answer:

$\large\boxed{\large\boxed{0.64M}}$

Explanation:

When you form a <em>diluted solution</em> from a mother (concentrated) solution, the moles of solute are determined by the mother solution.

The main equation is:

$Molarity=\dfrac{\text{moles of solute}}{\text{volume of the solution in liters}}$

Then, since the moles of solute is the same for both the mother solution and the diluted solution:

$\text{Molarity mother solution }\times\text{ volume mother solution}=\\\\=\text{Molarity diluted solution }\times\text{ volume diluted solution}$

Substitute and solve for the molarity of the diluted solution:

$250mL\times 0.75M=(45mL+250mL)\times M\\\\\\M=\dfrac{250mL\times 0.75M}{295mL}=0.64M$

8 0

3 years ago