All categories

3 years ago

Describe how an acidic solution forms when HCI is mixed in water

1 answer:

6 0

Acids are solutions with a high concentration of H+ ions. When HCl is put into water it dissociates. That means it breaks apart by the reaction:
HCl —> H+ + Cl-
One of the products of dissociation is H+, making the solution Acidic.

You might be interested in

Suppose that some FeSCN2+ is added to the above solution to shift the equilibrium. When equilibrium is re-established, the follo

kiruha [24]

Explanation:

The given reaction equation will be as follows.

$[FeSCN^{2+}] \rightleftharpoons [Fe^{3+}] + [SCN^{-}]$

Let is assume that at equilibrium the concentrations of given species are as follows.

$[Fe^{3+}] = 8.17 \times 10^{-3}$ M

$[SCN^{-}] = 8.60 \times 10^{-3}$ M

$[FeSCN^{2+}] = 6.25 \times 10^{-2}$ M

Now, first calculate the value of $K_{eq}$ as follows.

$K_{eq} = \frac{[Fe^{3+}][SCN^{-}]}{[FeSCN^{2+}]}$

= $\frac{8.17 \times 10^{-3} \times 8.60 \times 10^{-3}}{6.25 \times 10^{-2}}$

= $11.24 \times 10^{-4}$

Now, according to the concentration values at the re-established equilibrium the value for $[FeSCN^{2+}]$ will be calculated as follows.

$K_{eq} = \frac{[Fe^{3+}][SCN^{-}]}{[FeSCN^{2+}]}$

$11.24 \times 10^{-4} = \frac{8.12 \times 10^{-3} \times 7.84 \times 10^{-3}}{[FeSCN^{2+}]}$

$[FeSCN^{2+}] = 5.66 \times 10^{-2}$ M

Thus, we can conclude that the concentration of $[FeSCN^{2+}]$ in the new equilibrium mixture is $5.66 \times 10^{-2}$ M.

7 0

3 years ago

130cals.com

gregori [183]

Answer:x=3.76

Explanation:

6 0

2 years ago

What differs from between a radioactive isotope and a stable isotope

Digiron [165]

A stable isotope has just the right number of neutrons for the number of protons (the n:p ratio) to hold the nucleus together against the repulsions of the protons.

A radioactive isotope has either too few or too many neutrons for the nucleus to be stable,

The nucleus will then emit alpha, beta, or gamma radiation in an attempt to become more stable.

7 0

3 years ago

Write the overall, balanced molecular equation and indicate which element is oxidized and which is reduced for the following rea

REY [17]

Explanation:

Mg(s) + Cr(C2H3O2)3 (aq)

Overall, balanced molecular equation

Mg(s) + Cr(C2H3O2)3(aq) --> Mg(C2H3O2)3(aq) + Cr(s)

To identify if an element has been reduced or oxidized, the oxidation number is observed in both the reactant and product phase.

An increase in oxidation number denotes that the element has been oxidized.

A decrease in oxidation number denotes that the element has been reduced.

Oxidation number of Mg:

Reactant - 0

Product - +3

Oxidation number of Cr:

Reactant - +3

Product - 0

Note: C2H3O2 is actually acetate ion; CH3COO- The oxidatioon number of C, H and O do not change.

Oxidized : Mg

Reduced : Cr

7 0

3 years ago

How would you be able to tell if a train was moving?

lara [203]

Answer:

because I'm riding on it

8 0

3 years ago

Read 2 more answers