How much of each of the following substances would you add to water to prepare 1.90 L of a 0.15 M solution?

(a) H2SO4 from "concentrated" (18 M) sulfuric acid
mL
(b) HCl from "concentrated" (12 M) reagent
mL
(c) NiCl2 from the salt NiCl2·6 H2O
g
(d) HNO3 from "concentrated" (16 M) reagent
mL
(e) sodium carbonate from the pure solid
g
If u explained how to do one of them I should be able to do the rest. Thanks!

For solutions use the dilution formula of mL1 x M1 = mL2 x M2

For solids, calculate how many moles you need which is mols = M x L = 0.15 x 1.90 = ?
Then mols = grams/molar mass. You know mols and you have molar mass, solvel for grams.
Note that c wants Nicl2 but weighs NiCl2.6H2O. Since 1 mol NiCl2 is contained in 1 mol NiCl2.6H2O, use molar mass NiCl2.6H2O for this problem.

Well, aren't you demanding multiple substances all at once? You must be really thirsty for knowledge! Don't worry, I'm here to quench your curiosity!

Let's go step by step:

(a) To prepare 1.90 L of a 0.15 M H2SO4 solution, we can use the formula:

M1V1 = M2V2

Here, M1 is the initial concentration (18 M) and V1 is the volume we're trying to find (in mL). M2 is the final concentration (0.15 M) and V2 is the final volume (1.90 L).

First, let's convert the final volume to mL:

1.90 L = 1900 mL

Now, we can substitute the values and solve for V1:

(18 M)(V1) = (0.15 M)(1900 mL)

V1 = (0.15 M)(1900 mL) / (18 M)

V1 ≈ 15.8 mL

So, you'll need to add approximately 15.8 mL of concentrated sulfuric acid to the water.

Now it's your turn to give it a try for the others! Remember the secret formula M1V1 = M2V2, and let your chemistry skills sparkle!

To find the amount of each substance needed to prepare a 0.15 M solution in 1.90 L of water, you can use the formula:

Amount (in moles) = Concentration (in M) × Volume (in L)

(a) H2SO4 from "concentrated" (18 M) sulfuric acid:
To convert from moles to milliliters, you need to consider the molar mass of H2SO4: 98.09 g/mol.

Amount (in moles) = 0.15 M × 1.90 L = 0.285 moles
Volume (in mL) = Amount (in moles) × Molar mass (in g/mol) × 1000 mL/1 L
Volume (in mL) = 0.285 mol × 98.09 g/mol × 1000 mL/1 L = 27.952 mL

You would need to add 27.952 mL of 18 M sulfuric acid to prepare a 0.15 M solution in 1.90 L of water.

You can now follow the same steps to find the amounts for the remaining substances using their respective concentrations and molar masses:

(b) HCl from "concentrated" (12 M) reagent:
Amount (in moles) = 0.15 M × 1.90 L
Volume (in mL) = Amount (in moles) × Molar mass (in g/mol) × 1000 mL/1 L

(c) NiCl2 from the salt NiCl2·6 H2O:
Amount (in moles) = 0.15 M × 1.90 L
Mass (in g) = Amount (in moles) × Molar mass (in g/mol)

(d) HNO3 from "concentrated" (16 M) reagent:
Amount (in moles) = 0.15 M × 1.90 L
Volume (in mL) = Amount (in moles) × Molar mass (in g/mol) × 1000 mL/1 L

(e) Sodium carbonate from the pure solid:
Amount (in moles) = 0.15 M × 1.90 L
Mass (in g) = Amount (in moles) × Molar mass (in g/mol)

Just replace the concentration and molar mass values for each substance in the formulas above to find the required amounts in mL (for liquid solutions) or g (for solid substances).

To prepare a solution, you need to know the molar concentration of the solute (M) and the desired volume of the solution (L).

Here's how you can calculate the amount of each substance to add:

(a) H2SO4 from "concentrated" (18 M) sulfuric acid:
To calculate the volume needed (in mL), use the equation:
(0.15 M) × (V mL) = (18 M) × (1.90 L)
Solve for V mL.

(b) HCl from "concentrated" (12 M) reagent:
Using the same equation as above:
(0.15 M) × (V mL) = (12 M) × (1.90 L)
Solve for V mL.

(c) NiCl2 from the salt NiCl2·6H2O:
To calculate the mass needed (in g), you need to convert the molar concentration (M) to moles per liter (mol/L), then use the equation:
(0.15 mol/L) × (1.90 L) = (x mol) / (molar mass of NiCl2·6H2O)
Solve for x mol, then convert to grams using the molar mass.

(d) HNO3 from "concentrated" (16 M) reagent:
Using the same equation as above:
(0.15 M) × (V mL) = (16 M) × (1.90 L)
Solve for V mL.

(e) Sodium carbonate (Na2CO3) from the pure solid:
To calculate the mass needed (in g), you need first to convert molar concentration (M) to moles per liter (mol/L), then use the equation:
(0.15 mol/L) × (1.90 L) = (x mol) × (molar mass of Na2CO3)
Solve for x mol, then convert to grams using the molar mass.

For each calculation, substitute the known values and solve for the desired units of mL or g.