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Luba_88 [7]
3 years ago
6

What is the molarity of a solution that contains 17 g of nh3 in 0.50 l of solution?

Chemistry
1 answer:
Sauron [17]3 years ago
8 0

Answer:

  • 2.0 M

Explanation:

<u>1) Data:</u>

a) M = ?

b) mass of solue = 17 g

c) solute: NH₃

d) V = 0.5o liter

<u>2) Formulae:</u>

a) number of moles, n = mass in grams / molar mass

b) M = n / V (in liters)

<u>3) Solution</u>

a) Molar mass of NH₃ = 17.03 g/mol

b) n = mass in grams / molar mass = 17 g / 17.03 g/mol = 0.998 mol NH₃

c) M = n / V (in liters) = 0.998 mol / 0.50 liter = 1.996 M

d) Round to the appropiate number of significant figures, 2: 2.0 M.

Answer: 2.0 M

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A 1.0-L buffer solution is 0.10 M in HF and 0.050 M in NaF. Which action destroys the buffer? (a) adding 0.050 mol of HCl (b) ad
Volgvan

Answer:

(a) adding 0.050 mol of HCl

Explanation:

A buffer is defined as the mixture of a weak acid and its conjugate base -or vice versa-.

In the buffer:

1.0L × (0.10 mol / L) = 0.10 moles of HF -<em>Weak acid-</em>

1.0L × (0.050 mol / L) = 0.050 moles of NaF -<em>Conjugate base-</em>

-The weak acid reacts with bases as NaOH and the conjugate base reacts with acids as HCl-

Thus:

<em>(a) adding 0.050 mol of HCl:</em> The addition of 0.050moles of HCl produce the reaction of 0.050 moles of NaF producing HF. That means after the reaction, all NaF is consumed and you will have in solution just the weak acid <em>destroying the buffer</em>.

(b) adding 0.050 mol of NaOH: The NaOH reacts with HF producing more NaF. Would be consumed just 0.050 moles of HF -remaining 0.050 moles of HF-. Thus, the buffer <em>wouldn't be destroyed</em>.

(c) adding 0.050 mol of NaF: The addition of conjugate base <em>doesn't destroy the buffer</em>

3 0
3 years ago
What are the products of photosynthesis?
gtnhenbr [62]

Answer:

Glucose also called(Energy)

4 0
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Why is it illegal to manufacture fireworks without a license
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3 0
3 years ago
the atomic mass of N is 14.01 g/mol and the atomic mass of H is 1.008 g/mol. what is the molecular mass of NH3
nikdorinn [45]
Molecular mass= (14.01∗1)+(1.008∗3)
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7 0
3 years ago
A 0. 1220 g vitamin c tablet was dissolved in acid. This required 11. 50 ml of 0. 01740 m kio3 to reach the endpoint. Calculate
kodGreya [7K]

86.66 %  by weight of ascorbic acid in the tablet, when 0. 1220 g vitamin c tablet was dissolved in acid. This required 11. 50 ml of 0. 01740 m KIO_3 to reach the endpoint.

<h3>What is a balanced chemical equation?</h3>

A balanced chemical reaction is an equation that has equal numbers of each type of atom on both sides of the arrow.

3C_6H_80_6 +3I_2 +KIO_3 +5KI +6H^+ → 3C_6H_60_6 +6I^- +3I_2+6K^+ +3H_2O

So, the balanced chemical equation for the reaction will be:

3C_6H_8O_6 +KIO_3 → 3C_6H_6O_6 +KI + 3H_2O

That means, 3 mol of of ascorbic acid reacts with 1 mol of KIO_3

Moles of KIO_3 available is 0.0174 X 0.0115 =0.0002001 mol

Moles of ascorbic acid to be yielded should be 3 X 0.0002001 =0.0006003

So, percent mass of ascorbic acid in the tablet will be:

(0.1057 / 0.1220) X 100 %

=86.66 %

Hence, the third option is the correct answer.

Learn more about balanced chemical equations here:

brainly.com/question/26750249

#SPJ4

8 0
2 years ago
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