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Assoli18 [71]
3 years ago
8

What does it regulate? One sentence will help!

Chemistry
1 answer:
Mandarinka [93]3 years ago
7 0
<span>a regultate is to control or direct by a rule, principle, or method.</span>
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The balanced reaction between aqueous nitric acid and aqueous strontium hydroxide is _________
umka2103 [35]

Answer:

2HNO_3(aq)+Sr(OH)_2(aq)\rightarrow Sr(NO_3)_2(aq)+2H_2O(l)

Explanation:

Hello,

In this case, since nitric acid is HNO₃ and strontium hydroxide is Sr(OH)₂ we can represent the balanced chemical reaction by equaling the atoms of strontium, nitrogen, oxygen and hydrogen at both reactants and products as shown below:

2HNO_3(aq)+Sr(OH)_2(aq)\rightarrow Sr(NO_3)_2(aq)+2H_2O(l)

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What mass of FeSO4^2- x 6H20 (Molar Mass=260g/mol) is required to produce 500 mL of a .10M iron (II) sulfate solution.
lukranit [14]

Answer:

The correct option is: B. 13g

Explanation:

Given: Molar mass of iron (II) sulfate: m = 260g/mol,

Molarity of iron (II) sulfate solution: M =  0.1 M,

Volume of iron (II) sulfate solution: V = 500 mL = 500 × 10⁻³ = 0.5 L           (∵ 1L = 1000mL)

Mass of iron (II) sulfate taken: w = ? g

<em>Molarity</em>: M = \frac{n}{V (L)} = \frac{w}{m\times V(L)}

Here, n- total number of moles of solute, w - given mass of solute, m- molar mass of solute, V- total volume of solution in L

∴ <em>Molarity of iron (II) sulfate solution:</em>  M = \frac{w}{m\times V(L)}

⇒  w = M\times m\times V(L)

⇒  w = (0.1 M)\times (260g/mol)\times (0.5L)

⇒  <em>mass of iron (II) sulfate taken:</em> w = 13 g

<u>Therefore, the mass of iron (II) sulfate taken for preparing the given solution is 13 g.</u>

5 0
3 years ago
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