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3 years ago

#1: A concentration in terms of volume/volume is used to describe which of the following types of solutions?

2 answers:

5 0

B.
This method of expressing concentration is employed with solutions where both the solute and solvent are liquid. This is because it is easy to measure the volume of a liquid compared to that of a solid. Usually weight/weight is used in concentrations involving only solids.

laila [671]3 years ago

5 0

I believe the correct response would be D. Solutions with a liquid solvent and a solid solute. This is primarily for concentrations measured in terms of number of moles/volume.

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3 years ago

A 4.36 g sample of an unknown alkali metal hydroxide is dissolved in 100.0 ml of water. an acid-base indicator is added and the

Fofino [41]

Answer:

(a) $102.6g/mol$

(b) Rubidium

Explanation:

Hello,

This titration is carried out by assuming that the volume of base doesn't have a significant change when the mass is added, thus, we state the following data a apply the down below formula to compute the molarity of the base solution:

$V_{base}=0.1L; M_{acid}=2.5M, V_{acid}=0.017L\\V_{base}M_{base}=V_{acid}M_{acid}$

Solving for the molarity of base we've got:

$M_{base}=\frac{M_{acid}*V_{acid}}{V_{base}}=\frac{2.50M*0.017L}{0.1L} =0.425M=0.425mol/L$

Now, we can compute the moles of the base as:

$n_{base}=0.425mol/L*0.1L=0.0425mol$

(a) Now, one divides the provided mass over the previously computed moles to get the molecular mass of the unknown base:

$\frac{4.36g}{0.0425mol} =102.6g/mol$

(b) Subtracting the atomic mass of oxygen and hydrogen, the metal's atomic mass turns out into:

$102.6g/mol-16g/mol-1g/mol=85.6g/mol$

So, that atomic mass dovetails to the Rubidium's atomic mass.

Best regards.

8 0

3 years ago

What volume of 3.00 M HCl will form a solution with an acidic pH when mixed with 100 mL of 3.00 M NaOH

Maksim231197 [3]

Answer: The volume of acid should be less than 100 mL for a solution to have acidic pH

Explanation:

To calculate the volume of acid needed to neutralize, we use the equation given by neutralization reaction:

$n_1M_1V_1=n_2M_2V_2$

where,

$n_1,M_1\text{ and }V_1$ are the n-factor, molarity and volume of acid which is HCl

$n_2,M_2\text{ and }V_2$ are the n-factor, molarity and volume of base which is NaOH

We are given:

$n_1=1\\M_1=3.00M\\V_1=?mL\\n_2=1\\M_2=3.00M\\V_2=100mL$

Putting values in above equation, we get:

$1\times 3.00\times V_1=1\times 3.00\times 100\\\\V_1=\frac{1\times 3.00\times 100}{1\times 3.00}=100mL$

For a solution to be acidic in nature, the pH should be less than the volume of acid needed to neutralize.

Hence, the volume of acid should be less than 100 mL for a solution to have acidic pH

7 0

3 years ago