Question

A couple of questions...Thank you for anyone that replies.

#1 For the following (unbalanced) reaction, what is the salt?

H₃PO₄ + NaOH --> Na₃PO₄ + HOH

#2 For the following (unbalanced) reaction, what is the base?

H₃PO₄ + NaOH --> Na₃PO₄ + HOH

#3 For the following reaction, what is the base?

NaF + HCl-- > NaCl + HF

#4 What are the oxidation numbers on O in SO₂, in O₂, and in SO₃?

How many ml of 1.06M sulfuric acid would be necessary to completely neutralize 59.9ml of 3.86M NaOH?

Answer 1

#1 For the equation given, the salt in the reaction is,

Na3PO4

#2 For the given reaction, the base is,

NaOH

#3 For the given reaction, the base in reaction is,

NaF

#4 the oxidation number of,

O in SO2

let x be the oxidation number for O

4 + x = 0

x = -4

For O in O2

oxidation number is 0

For O in SO3,

oxidation number = -2

#5 The chemical equation for neutralizaton would be,

H2SO4 + 2NaOH ---> Na2SO4 + 2H2O

So 1 mole of H2SO4 neutralized 2 moles of NaOH

moles of NaOH = molarity x volume = 3.86 x 59.9 = 231.214 mmoles

So, moles of H2SO4 = 231.214/2 = 115.607 mmoles

mL of H2SO4 required = 115.607/1.06 = 109.063 mL