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3 years ago

PORFA AYUDAA !!!

Chemistry

1 answer:

matrenka [14]3 years ago

6 0

Explanation:

The problem here is to find the atomic number of each of the element given.

Sum the powers of the configuration.

a- 1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹

Atomic number is = 2 + 2 + 6 + 2 + 6 + 1 = 19

b- 1s² 2s² 2p⁶ 3s² 3p⁴

Atomic number = 2 + 2 + 6 + 2 + 4 = 16

c- 1s¹

Atomic number = 1

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Which represents the self ionization of water at 25 degrees

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This question comes with four answer choices:

A. H2O + H2O ⇄ 2H2 + O2

B. H2O + H2O⇄ H2O2 + H2

C. H2O + H2O ⇄ 4H+ + 2O2-

D. H2O + H2O ⇄ H3O+ + OH-

Answer: option D. H2O + H2O ⇄ H3O+ + OH-

(the +sign next to H3O is a superscript, as well as the - sing next to OH)

Explanation:

The self-ionization of water, or autodissociation, produces the two ions H3O(+) and OH(-). The presence of ions is what explain the electrical conductivity of pure water.

In this, one molecule of H2O loses a proton (H+) (deprotonates) to become a hydroxide ion, OH−. Then, he hydrogen ion, H+, immediately protonates another water molecule to form hydronium, H3O+.

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azamat

Answer : The value of $K_{sp}$ for $BaCO_3$ is $19.36\times 10^{-10}mole^2/L^2$ .

Solution : Given,

Solubility of $BaCO_3$ in water = $4.4\times 10^{-5}mole/L$

The barium carbonate is insoluble in water, that means when we are adding water then the result is the formation of an equilibrium reaction between the dissolved ions and undissolved solid.

The equilibrium equation is,

$BaCO_3\rightleftharpoons Ba^{2+}+CO^{2-}_3$

Initially - 0 0

At equilibrium - s s

The Solubility product will be equal to,

$K_{sp}=[Ba^{2+}][CO^{2-}_3]$

$K_{sp}=s\times s=s^2$

$[Ba^{2+}]=[CO^{2-}_3]=s=4.4\times 10^{-5}mole/L$

Now put all the given values in this expression, we get the value of solubility constant.

$K_{sp}=(4.4\times 10^{-5}mole/L)^2=19.36\times 10^{-10}mole^2/L^2$

Therefore, the value of $K_{sp}$ for $BaCO_3$ is $19.36\times 10^{-10}mole^2/L^2$ .

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