Can anyone help me with this question

How much NaCl should be added to 0.35 L of a 0.15 M solution of AgNO3 so that it reacts completely with the silver to form AgCl(s)?
A. 8.8 g
B. 0.0525 g
C. 0.89 mg
D. 3.07 g

3.07 g

Well, it looks like you're in a bit of a NaCl-ing situation! Don't worry, I'm here to help you add some sodium chloride to the mix.

To figure out how much NaCl you need, let's use the balanced chemical equation for the reaction between AgNO3 and NaCl: AgNO3 + NaCl -> AgCl(s) + NaNO3.

First, let's calculate the number of moles of AgNO3 in the given solution:
moles of AgNO3 = volume of solution (L) x molarity of AgNO3 (mol/L)
moles of AgNO3 = 0.35 L x 0.15 mol/L
moles of AgNO3 = 0.0525 mol

Since the reaction is 1:1 between AgNO3 and NaCl, you will need the same number of moles of NaCl to react completely.

Now, let's find the mass of NaCl needed:
mass of NaCl (g) = moles of NaCl x molar mass of NaCl (g/mol)
mass of NaCl (g) = 0.0525 mol x 58.44 g/mol
mass of NaCl (g) = 3.0678 g

So, the answer is D. You will need approximately 3.07 grams of sodium chloride to react completely with the silver in the solution. Just make sure to weigh it out carefully and clown around while you're at it!

To find out how much NaCl should be added to react with the silver in the AgNO3 solution, you can use stoichiometry and the balanced equation for the reaction between AgNO3 and NaCl:

AgNO3(aq) + NaCl(aq) -> AgCl(s) + NaNO3(aq)

From the balanced equation, you can see that the stoichiometric ratio of AgNO3 to NaCl is 1:1. Therefore, for every 1 mole of AgNO3, you would need 1 mole of NaCl.

Step 1: Calculate the number of moles of AgNO3 in the solution.

Moles = concentration (M) x volume (L)
Moles of AgNO3 = 0.15 M x 0.35 L

Step 2: Convert the moles of AgNO3 to moles of NaCl.

Since the stoichiometric ratio of AgNO3 to NaCl is 1:1, the moles of NaCl will be the same as the moles of AgNO3.

Step 3: Calculate the mass of NaCl needed.

Mass = moles x molar mass
Mass of NaCl = moles of NaCl x molar mass of NaCl

The molar mass of NaCl is 58.44 g/mol.

Step 4: Convert the mass of NaCl to the appropriate unit from the given answer choices.

Now, let's plug in the numbers:

Moles of AgNO3 = 0.15 M x 0.35 L = 0.0525 mol
Moles of NaCl = 0.0525 mol
Mass of NaCl = 0.0525 mol x 58.44 g/mol = 3.0658 g

Comparing the calculated mass to the given answer choices, we can see that the closest option is option D, 3.07 g.

Therefore, the correct answer is D. 3.07 g

To determine how much NaCl should be added to react completely with the silver in the solution, we need to use stoichiometry and the balanced chemical equation for the reaction.

The balanced chemical equation for the reaction between AgNO3 and NaCl is:

AgNO3 + NaCl -> AgCl + NaNO3

From the balanced equation, we can see that 1 mole of AgNO3 reacts with 1 mole of NaCl to form 1 mole of AgCl.

To start, we need to convert the volume of the AgNO3 solution to moles. We will use the formula:

Moles = Concentration x Volume

Moles of AgNO3 = 0.15 M x 0.35 L
Moles of AgNO3 = 0.0525 moles

Since 1 mole of AgNO3 reacts with 1 mole of NaCl, we need an equal number of moles of NaCl to react completely. So, the number of moles of NaCl needed is also 0.0525 moles.

Next, we need to convert moles of NaCl to grams using the molar mass of NaCl. The molar mass of NaCl is 58.44 g/mol.

Mass of NaCl = Moles x Molar Mass
Mass of NaCl = 0.0525 moles x 58.44 g/mol
Mass of NaCl = 3.07 g

Therefore, the correct answer is D. 3.07 g.

Write down the reaction:

NaCl + Ag(+) ---> AgCl + Na(+)

The main thing to note here is that 1 mol of NaCl reacts completely with 1 mol of silver to form the required product.

How many moles of Ag do we have?
(It will be equal to the number of moles of AgNO3, since one mole of silver nitrate contains one mole of silver)

Molarity = (number of moles)/(volume of solution)
(number of moles) = (Molarity) * (volume)
= (0.15) * (0.35)

When you solve this, you will get the number of moles of AgNO3. This will be equal to the number of moles of Ag in the solution, and the number of moles of NaCl to be added.

Given the number of moles of NaCl, can you convert this into the mass required?