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solmaris [256]
3 years ago
7

A student needs to prepare 100. mL of 0.612 M Cu(NO3)2 solution. What mass, in grams, of copper(II) nitrate should the student u

se? Enter a numerical value with the correct number of significant figures in the answer box. Do not enter units, but know that the final units must be grams.
Chemistry
1 answer:
Temka [501]3 years ago
3 0

Answer: 11.5 grams

Explanation:

Molarity of a solution is defined as the number of moles of solute dissolved per Liter of the solution

Molarity=\frac{n\times 1000}{V_s}

where,

Morality = 0.612 M

n= moles of solute  

V_s = volume of solution in ml = 100 ml

Now put all the given values in the formula of molarity, we get

0.612=\frac{n\times 1000}{100ml}

n=0.0612moles

Mass={\text {moles of solute }}{\times {\text {molar mass}}=0.0612moles\times 187.56g/mol=11.5g

Therefore, the mass of copper (II)nitrate required is 11.5 grams

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Question 231.15 pts A 0.200 M solution of a weak monoprotic acid HA is found to have a pH of 3.00 at room temperature. What is t
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Answer:

The correct answer is: Ka= 5.0 x 10⁻⁶

Explanation:

The ionization of a weak monoprotic acid HA is given by the following equilibrium: HA ⇄ H⁺ + A⁻. At the beginning (t= 0) we have 0.200 M of HA. Then, a certain amount (x) is dissociated into H⁺ and A⁻, as is detailed in the following table:

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t              -x                             x                       x

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At equilibrium, we have the following ionization constant expression (Ka):

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