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il63 [147K]
3 years ago
15

A buffer is prepared by dissolving 0.80 moles of NH3 and 0.80 moles of NH4Cl in 1.00 L of aqueous solution. If 0.10 mol of NaOH

is added to 250 mL of this buffer, what is the pH of the resultant solution?
a.10.54
b.4.27
c.8.78
d.9.73
e.5.22
Chemistry
1 answer:
Vikki [24]3 years ago
7 0

Answer:

a. 10.54

Explanation:

reaction is

NH₃ +  NaOH   -----------------NH₄Cl + H₂O

0.10 mol NaOH will consume 0.10 mol NH₃ thereby decreasing the initial amount of moles NH₃ and increasing that of NH₄Cl

mol NH₃  = 0.80 - 010 = .70

mol NH₄Cl = 0.80 + .10 = 0.90

pH = pKₐ + log (( NH₃/NH₄Cl))

pH =  9.26 + log (( 0.90 + 0.70)) = 9.26 + 0.11 = 10.54

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Answer:

4

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How many moles of hydrogen are in 3. 06 × 10⁻³ g of glycine , c₂h₅no₂?.
Gala2k [10]

Answer:

n = 6.06 x 10^{-4} mol

Explanation:

n =?

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Atomic mass of H is 1,01, etc.

Having this data, we can use the Molar mass formula and change it so we can know the quantity of matter (n) in moles, and we just replace it.

M = \frac{m}{n} ⇔ n = \frac{m}{M} ⇔ n = \frac{3.06 x 10^{-3} }{5,05} ⇔ n = 6.06 x 10^{-4} mol

Note: The numbers I've used may be different from yours, by a small difference. I don't know if it's the case, but hope it helped.

8 0
2 years ago
Dichlorine monoxide, Cl2O is sometimes used as a powerful chlorinating agent in research. It can be produced by passing chlorine
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Answer:

% yield =  82.5%

Explanation:

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Our reactants are:

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Our products are:

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We do not have information about moles of reactants, but we do know the theoretical yield and the grams of product, in this case Cl₂O, we have produced.

Percent yield = (Yield produced / Theoretical yield) . 100

Theoretical yield is the mass of product which is produced by sufficent reactant. We replace data:

% yield = (0.71 g/0.86g) . 100 = 82.5%

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Answer:

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