Find the volume of 0.240 m sulfuric acid necessary to react completely with 72.8 g sodium hydroxide. express your answer with the appropriate units.

The volume neccesary to complete reaction is 3.79L

Explanation:

First step: Think the equation

H2SO4 + 2NaOH →  Na2SO4  + 2H2O

Afterwards, ballance it.

Relation in reactants is 1:2, so 2 mol of NaOH react to 1 mol of sulfuric.

Gotta find my mol of NaOH

Mass / Molar weight = Mol

72.8 g / 40 g/m = 1.82 mol NaOH

As the relation is 1:2, I have the half of sulfuric: 0.91 mol.

By a rule of three, will be

2 mol NaOH __ react __ 1 mol H2SO4

1.82 mol NaOH __react ___ (1.82 .1)/2

Finally we have to work with molarity, which means mol/L. So, the rule of three is:

0.240 mol H2SO4 __are in __ 1 L

0.91 mol H2SO4___ are in ___ (0.91  .1)/0.240 = 3.79L

explanation:

let the different atoms be x and y. each with four protons and same mass will be represented as follows.

mass number is number of protons + number of neutrons.

            and  

since, it is given that one has a negative charge while the other is neutral. therefore, there will be increase in number of protons and the atom will be represented as follows.

according to periodic table, mass number of beryllium is 9 and it has atomic number 4 so, the atoms will be and .  

the protons and neutrons will be located inside the nucleus whereas the electrons will be revolving around the nucleus.