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3 years ago

Examine the following false statement.

Chemistry

2 answers:

riadik2000 [5.3K]3 years ago

6 0

Answer:

The first one

Explanation:

It's the opposite of the false statement

ArbitrLikvidat [17]3 years ago

5 0

Answer:

Acids that partially dissociate are weak acids, while acids that fully dissociate are strong acids.

Explanation:

The pH scale range from 0 to 14. A pH of 7 is neutral; below it is acidic while a pH above 7 is basic.

While low pH might be an indication of a strong acid, a high pH on the pH scale indicates a base or alkaline.

<em>On the other hand, when it comes to the degree of ionization in water, a strong acid is the one that completely ionizes in water while a weak acid partially ionizes in water.</em>

Hence, of all the available options, only the second option correctly describes acids.

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An aqueous solution of sodium fluoride is slowly added to a water sample that contains barium ion (2.75×10-2M ) and calcium ion

Alona [7]

Answer : The remaining concentration of the first ion to precipitate when the second ion begins to precipitate is, $1.07\times 10^{-6}M$

Explanation :

The dissociation of barium fluoride is written as:

$BaF_2\rightleftharpoons Ba^{2+}+2F^-$

The expression for solubility constant for this reaction will be,

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

As we know that at room temperature $25^oC$ the $K_{sp}$ of barium fluoride is, $1\times 10^{-6}$ .

Now put all the given values in this expression, we get:

$1\times 10^{-6}=(2.75\times 10^{-2})\times [F^-]^2$

$[F^-]=6.03\times 10^{-3}M=0.00603M$

The barium fluoride precipitate when fluoride ion is equal to 0.00603 M.

The dissociation of calcium fluoride is written as:

$CaF_2\rightleftharpoons Ca^{2+}+2F^-$

The expression for solubility constant for this reaction will be,

$K_{sp}=[Ca^{2+}][F^-]^2$

As we know that at room temperature $25^oC$ the $K_{sp}$ of calcium fluoride is, $3.90\times 10^{-11}$ .

Now put all the given values in this expression, we get:

$3.90\times 10^{-11}=(6.70\times 10^{-2})\times [F^-]^2$

$[F^-]=2.41\times 10^{-5}M=0.0000241M$

The calcium fluoride precipitate when fluoride ion is equal to 0.0000241 M.

Since, the fluoride ion concentration in calcium fluoride is less then the fluoride ion concentration in barium fluoride. That means, calcium fluoride will precipitate first.

Thus, the concentration $Ca^{2+}$ ion remaining at $F^-$ concentration (0.00603 M) is calculated as:

$K_{sp}=[Ca^{2+}][F^-]^2$

Now put all the given values in this expression, we get:

$3.90\times 10^{-11}=[Ca^{2+}]\times (0.00603)^2$

$[Ca^{2+}]=1.07\times 10^{-6}M$

Therefore, the remaining concentration of the first ion to precipitate when the second ion begins to precipitate is, $1.07\times 10^{-6}M$

3 0

3 years ago

Why Is it important to have exact standards of measurement ?

notsponge [240]

A standard of measurement system is important because it allows scientists to compare data and communicate with each other about their results.

3 0

3 years ago

Pls help i need help with science what is the name of all satruns moons?

pantera1 [17]

Answer:

here look at the image

Explanation:

5 0

2 years ago

What is the effect of adding heat to a gas at constant pressure?

Anna007 [38]

The pressure will continue to build up eventually causing a release of pressure or an explosion.

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3 years ago

Compare the value you calculated for the number of sand grains on Earth’s beaches to the number of particles in a mole. What can

Wewaii [24]

Answer:

6.022×1023 particles are present in one mole of a substance while about 7.5 x 1018 grains of sand are present on earth's beaches.

Explanation:

Mole is used in chemistry for the calculation of mass of an atom. 6.022×1023 particles are present in one mole of a substance while about 7.5 x 1018 grains of sand are present on earth's beaches. According to this data which shows that the size of mole is greater than the number of sand grains present on Earth’s beaches because there are higher particles are present in mole as compared to sand grains. So the mole has big size.

6 0

3 years ago

Read 2 more answers