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IrinaK [193]
3 years ago
10

Bi2(CO3)3 Name of this compound

Chemistry
1 answer:
Keith_Richards [23]3 years ago
5 0

Answer:

The name of this compound is :

Bi2(CO3)3 = Bismuth Carbonate

Explanation:

The name of the compound is derived from the name of the elements present  in it.

The rule followed while naming the compound are:

1. The first element (always the cation) is named as such .

2. The second element (The anion) end with "-ate ,  -ide ," etc

3. NO prefix is added while naming the first element.

For example : Bi2 can't be named as Dibismuth

Na2 = Can't be named as disodium

Hence the compound :

Bi2(CO3)3 contain two element : Bi and CO3. Here , Bi = cation (named as such) and CO3 = anion (named according to rules)

Bi = Bismuth

CO3 = carbonate

Bi2(CO3)3 = Bismuth Carbonate

The molecular mass of this compound is :

Molecular mass = 2 (mass of Bi) + 3(mass of C) + 6(mass of O)

= 2 (208.98)+3(12.01)+6(15.99)

= 597.987 u

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Will a precipitate of magnesium fluoride form when 300. mL of 1.1 × 10 –3 M MgCl 2 are added to 500. mL of 1.2 × 10 –3 M NaF? [K
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Answer:

No precipitate is formed.

Explanation:

Hello,

In this case, given the dissociation reaction of magnesium fluoride:

MgF_2(s)\rightleftharpoons Mg^{2+}+2F^-

And the undergoing chemical reaction:

MgCl_2+2NaF\rightarrow MgF_2+2NaCl

We need to compute the yielded moles of magnesium fluoride, but first we need to identify the limiting reactant for which we compute the available moles of magnesium chloride:

n_{MgCl_2}=0.3L*1.1x10^{-3}mol/L=3.3x10^{-4}molMgCl_2

Next, the moles of magnesium chloride consumed by the sodium fluoride:

n_{MgCl_2}^{consumed}=0.5L*1.2x10^{-3}molNaF/L*\frac{1molCaCl_2}{2molNaF} =3x10^{-4}molMgCl_2

Thus, less moles are consumed by the NaF, for which the moles of formed magnesium fluoride are:

n_{MgF_2}=3x10^{-4}molMgCl_2*\frac{1molMgF_2}{1molMgCl_2}=3x10^{-4}molMgF_2

Next, since the magnesium fluoride to magnesium and fluoride ions is in a 1:1 and 1:2 molar ratio, the concentrations of such ions are:

[Mg^{2+}]=\frac{3x10^{-4}molMg^{+2}}{(0.3+0.5)L} =3.75x10^{-4}M

[F^-]=\frac{2*3x10^{-4}molMg^{+2}}{(0.3+0.5)L} =7.5x10^{-4}M

Thereby, the reaction quotient is:

Q=(3.75x10^{-4})(7.5x10^{-4})^2=2.11x10^{-10}

In such a way, since Q<Ksp we say that the ions tend to be formed, so no precipitate is formed.

Regards.

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Answer:

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