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3 years ago

Positive ions from a base and negative ions from an acid form a_____ .

Chemistry

2 answers:

lara31 [8.8K]3 years ago

5 0

They will form a Salt

Anna35 [415]3 years ago

4 0

Explanation:

Bases are the species which contain $OH^{-}$ ions whereas acids are the species which contain $H^{+}$ ions. When positive ions from a base reacts with negative ions of an acid then it results in the formation of salt.

For example, when base NaOH reacts with hydrochloric acid then it results in the formation of sodium chloride and water.

The reaction is as follows.

$NaOH + HCl \rightarrow NaCl + H_{2}O$

Thus, we can conclude that positive ions from a base and negative ions from an acid form a salt.

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For the equation PV = nRT, re-write it so that it is in the form of "T = ".

mamaluj [8]

T=PV/nR
that is the answer

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3 years ago

What mass of TiCl4 must react with an excess of water to produce 50.0g of TiO2 if the reaction has a 78.9% yield

Kipish [7]

Answer:

\large \boxed{\text{150 g TiCl}_{4}}

Explanation:

We will need a balanced chemical equation with masses and molar masses, so, let's gather all the information in one place.

Mᵣ: 189.68 79.87

TiCl₄ + 2H₂O ⟶ TiO₂ + 4HCl

m/g: 50.0

To solve this stoichiometry problem, you must

Convert the actual yield to the theoretical yield
Use the molar mass of TiO₂ to convert the theoretical yield of TiO₂ to moles of TiO₂
Use the molar ratio to convert moles of TiO₂ to moles of TiCl₄
Use the molar mass of TiCl₄ to convert moles of TiCl₄ to mass of TiCt₄

1. Theoretical yield of TiO₂

$\text{Theoretical yield} = \text{50.0 g actual} \times \dfrac{\text{100 g theoretical}}{\text{78.9 g actual}} = \text{63.37 g theoretical}$

2. Moles of TiO₂

$\text{Mass of TiO}_{2} = \text{63.37 g TiO}_{2} \times \dfrac{\text{1 mol TiO}_{2}}{\text{79.87 g TiO}_{2} } = \text{0.7934 mol TiO}_{2}$

3, Moles of TiCl₄

The molar ratio is 1 mol TiO₂:1 mol TiCl₄.

$\text{Moles of TiCl}_{4} = \text{0.7934 mol TiO}_{2} \times \dfrac{\text{1 mol TiCl}_{4}}{\text{1 mol TiO}_{2}} = \text{0.7934 mol TiCl}_{4}$

4. Mass of TiCl₄

$\text{Mass of TiCl}_{4} = \text{0.7934 mol TiCl}_{4} \times \dfrac{\text{189.98 g TiCl}_{4}}{\text{1 mol TiCl}_{4}} =\textbf{150 g TiCl}_{\mathbf{4}} \\\\\text{You must use $\large \boxed{\textbf{150 g TiCl}_{\mathbf{4}}}$}$

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3 years ago

How long will it take Barium-142 to decay to 25% of its original size?

Leya [2.2K]

Answer:

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Explanation:

just divide. hope this helps!

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Svet_ta [14]

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Harman [31]

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3 years ago