Titration of a weak acid with a strong base. the ph curve for titration of 50.0ml of a 0.100 M of acetic acid with a 0.100 M solution of NaOH (aq). For clarity, water molecules have been omitted from the molecular art.

a) If the acetic acid being titrated here were replaced by hydrochloric acid, would the amount of base needed to reach the equivalence point change?

b) Would the pH at the equivalence point change?
a. yes the pH at the equivalence point will increase.
b. yes the pH at the equivalence point will decrease.
c. no the pH will not change

CH4 + 2O2 > CO2 + 2H2O

Explanation:

What are the rules in balancing chemical equations

1 . Write the correct chemical formulas for all the reactants and products

2. Count the total number of atoms or ions of each element in the reactants and also of the product

3. Balance the elements one at a time using coefficient

4. Check each atoms or ions to ensure correctly balanced

5. Make sure that all the coefficient are in the lowest possible whole number ratio

CH4 + O2 > CO2 + H2O

reactant. Product

Write out each number of atoms of each element for both the reactant and the product

Reactant. Product

1 C 1C

4H 2H

2O 3O

balance each element at a time

CH4 + O2 > CO2 + H2O

let's balance H2O by adding coefficient of 2

CH4 + O2 > CO2 +2 H2O

since :H - 4 at the reactant and also at the product

: O - 4 at the product but 2 at the reactant

Let's add the coefficient of 2 to O to balance the equation

CH4 + 2O2 > CO2 + 2H2O

C. C

4H. 4H

4O. 2O + 2O = 4O

so our chemical equation is balanced

CH4 + 2O2 > CO2 + 2H2O