<u>Answer:</u> The concentration of solution is 0.342 M
<u>Explanation:</u>
To calculate the molarity of solution, we use the equation:

We are given:
Mass of solute (Sodium chloride) = 15 g
Molar mass of sodium chloride = 58.5 g/mol
Volume of solution = 750 mL
Putting values in above equation, we get:

Hence, the concentration of solution is 0.342 M
<u>Answer:</u> The correct answer is Option 5.
<u>Explanation:</u>
- To calculate the molarity of the solution after mixing 2 solutions, we use the equation:

where,
are the n-factor, molarity and volume of the NaOH.
are the n-factor, molarity and volume of the 
We are given:
Putting all the values in above equation, we get:

- To calculate the molarity of acid, we use the equation given by neutralization reaction:

where,
are the n-factor, molarity and volume of acid which is 
are the n-factor, molarity and volume of base.
We are given:

Putting values in above equation, we get:

Hence, the correct answer is Option 5.
What are the answer choices?
Answer:

Explanation:
Hello,
In this case, the undergoing chemical reaction is:

Thus, for 0.904 g of precipitate, that is lead (II) iodide, we can compute the initial moles of lead (II) ions in lead (II) nitrate:

Finally, the resulting molarity in 30.8 mL (0.0308 L):

Regards.
False
The adjective corrosive means it will definitely harm the skin