the balance equation for the reaction of aqueous sulfuric acid with aqueous ammonia is

2NH3(aq)+ H2SO4(aq) -> (NH4)2SO4(aq)

1. what volume of 0.250M sulfuric acid solution would be needed to react completely with 18.00mL of 0.350M ammonia solution?

2. what mass of ammonium sulfate would be formed by this reaction?

1. Well, isn't this a fun chemical party! Let's do some calculations. We know that the balanced equation is 2NH3(aq) + H2SO4(aq) -> (NH4)2SO4(aq). According to the stoichiometry, we need 2 moles of ammonia for every 1 mole of sulfuric acid.

To find the volume of sulfuric acid needed, let's use a little math magic. We have 18.00 mL of a 0.350 M ammonia solution. That means we have (0.350 M)*(0.01800 L) = 0.00630 moles of ammonia.

Since we need 2 moles of ammonia for every 1 mole of sulfuric acid, we divide 0.00630 moles by 2 to find the number of moles of sulfuric acid needed. That gives us 0.00315 moles of sulfuric acid.

Now, we can use the concentration of the sulfuric acid solution to find the volume needed. We have a 0.250 M sulfuric acid solution, so we divide 0.00315 moles by 0.250 M to get the volume in liters. That gives us 0.0126 L, or 12.6 mL.

So, you would need approximately 12.6 mL of the 0.250 M sulfuric acid solution to react completely with 18.00 mL of the 0.350 M ammonia solution.

2. Now, let's calculate the mass of ammonium sulfate formed. We need to find the number of moles of ammonium sulfate formed, and then multiply it by its molar mass.

From the balanced equation, we can see that 1 mole of (NH4)2SO4 is formed for every 1 mole of H2SO4. So, the number of moles of (NH4)2SO4 formed will be the same as the number of moles of sulfuric acid used, which is 0.00315 moles.

The molar mass of (NH4)2SO4 is 132.14 g/mol, so we can multiply the number of moles by the molar mass to find the mass of (NH4)2SO4 formed:
0.00315 moles * 132.14 g/mol = 0.416 g

Therefore, the mass of ammonium sulfate formed by this reaction is approximately 0.416 grams.

To answer these questions, we will use the principles of stoichiometry and the balanced chemical equation provided.

1. First, we need to determine the moles of ammonia and sulfuric acid used in the reaction.

Given:
- Volume of ammonia solution = 18.00 mL = 0.01800 L
- Molarity of ammonia solution = 0.350 M

The moles of ammonia can be calculated using the formula:

moles = volume (L) x molarity

moles of NH3 = 0.01800 L x 0.350 M
moles of NH3 = 0.00630 mol

According to the balanced equation, the ratio between ammonia and sulfuric acid is 2:1. Therefore, the moles of sulfuric acid required will be half of the moles of ammonia used:

moles of H2SO4 = 0.00630 mol / 2
moles of H2SO4 = 0.00315 mol

Now we can calculate the volume of the sulfuric acid solution required.

Given:
- Molarity of sulfuric acid solution = 0.250 M

Using the formula:

volume (L) = moles / molarity

volume of H2SO4 = 0.00315 mol / 0.250 M
volume of H2SO4 = 0.0126 L or 12.6 mL

Therefore, approximately 12.6 mL of 0.250 M sulfuric acid solution would be needed to react completely with 18.00 mL of 0.350 M ammonia solution.

2. To determine the mass of ammonium sulfate formed in this reaction, we need to use the stoichiometric ratio between ammonium sulfate and sulfuric acid.

According to the balanced equation, the ratio between NH4HSO4 and H2SO4 is 1:1. Therefore, the moles of ammonium sulfate formed will be equal to the moles of sulfuric acid used:

moles of (NH4)2SO4 = moles of H2SO4
moles of (NH4)2SO4 = 0.00315 mol

Given:
- Molar mass of (NH4)2SO4 = 132.14 g/mol

Using the formula:

mass = moles x molar mass

mass of (NH4)2SO4 = 0.00315 mol x 132.14 g/mol
mass of (NH4)2SO4 = 0.417 g

Therefore, approximately 0.417 grams of ammonium sulfate would be formed by this reaction.

To answer these questions, we need to use stoichiometry and the given molar concentrations of the solutions.

1. To determine the volume of sulfuric acid solution needed, we will first write a balanced equation for the reaction:

2NH3(aq) + H2SO4(aq) -> (NH4)2SO4(aq)

The balanced equation tells us that 2 moles of ammonia react with 1 mole of sulfuric acid to produce 1 mole of ammonium sulfate. Now, we can use stoichiometry:

Given:
- Volume of ammonia solution = 18.00 mL = 0.018 L
- Molarity of ammonia solution = 0.350 M

We can calculate the moles of ammonia in the given volume:
moles of NH3 = volume (in L) x molarity
moles of NH3 = 0.018 L x 0.350 M = 0.0063 moles

According to the balanced equation, 2 moles of ammonia react with 1 mole of sulfuric acid. Therefore, we need half as many moles of sulfuric acid:

moles of H2SO4 = (1/2) x moles of NH3
moles of H2SO4 = (1/2) x 0.0063 moles = 0.00315 moles

Now we can calculate the volume of sulfuric acid solution needed:
volume of H2SO4 solution = moles of H2SO4 ÷ molarity
volume of H2SO4 solution = 0.00315 moles ÷ 0.250 M = 0.0126 liters = 12.6 mL

Therefore, approximately 12.6 mL of 0.250M sulfuric acid solution is needed to completely react with 18.00 mL of 0.350M ammonia solution.

2. To find the mass of ammonium sulfate formed, we will use the equation again:

2NH3(aq) + H2SO4(aq) -> (NH4)2SO4(aq)

According to the balanced equation, 2 moles of ammonia react to produce 1 mole of ammonium sulfate.

From part 1, we found that the number of moles of ammonia is 0.0063 moles. Hence, the number of moles of ammonium sulfate formed will be half that amount:

moles of (NH4)2SO4 = (1/2) x moles of NH3
moles of (NH4)2SO4 = (1/2) x 0.0063 moles = 0.00315 moles

To calculate the mass of ammonium sulfate formed, we need to multiply the number of moles by its molar mass. The molar mass of (NH4)2SO4 is 132.14 g/mol:

mass of (NH4)2SO4 = moles of (NH4)2SO4 x molar mass
mass of (NH4)2SO4 = 0.00315 moles x 132.14 g/mol = 0.416 g

Therefore, approximately 0.416 grams of ammonium sulfate will be formed by this reaction.

1. mols NH3 = M x L = ?

Using the coefficients in the balanced eqauation, convert mols NH3 to mols
H2SO4.
Now M H2SO4 = mols/L, You know mols and M, solve for L and convert to mL if needed.

2.
You have mols NH3. Using the coefficients convert mols NH3 to mols (NH4)2SO4.
Now convert mols to g. g = mols x molar mass