Suppose you wanted to produce 1.00 L of 3.50 M solution of H2SO4. How many grams of the solute are needed to make this solution?

343g H2SO4

Explanation

1. H2SO4 is the solute

2. Water is the solvent

3. Molarity = moles of solute / liter of solution = n / V

(Note the case of the letters is important in science. N stands for Normal in chemistry a type of concentration, n stands for the number of moles)

Rearrange the formula to find n

n = M x V

Here are the known values,

M = 3.5M

n = x mol

V = 1.00L

Plug it in and solve for n (the number of moles of H2SO4 in the solution)

n = 3.5M x 1.00 L = 3.50 mol of H2SO4

Molecular mass of H2SO4 is 1g/mole H x 2 + 32.1g/mol S + 16g/mol O x 4 = 98.1g/mol H2SO4

mass = number of mole x relative molecular mass

mass = n x 98.1g/mol

mass = 98.1g/mol H2SO4 x 3.50mol H2SO4

= 343g H2SO4 <-answer

answer: c. the experiment shows that the red substance experienced a chemical change.

explanation: chemical change is the change in which chemical composition of the substance changes. physical change is the change in which there is no change in chemical composition.

chemical changes are accompanied by following changes:

a) precipitate formation

b) energy is released or absorbed

c) formation of bubbles

d) change in color

as it is given that the red color has disappeared and there is production of gas, it means the red substance has undergone a chemical change.

e

the ratio of the conjugate base to the acid required to attain the desired ph.