Part A; A stronger solution of sodium bicarbonate require more hydrochloric acid will be required
Part A; The reason why more HCl is required is due to the presence of more hydroxyl ions in the solution
The reason arriving at the above responses are as follows;
Part A
Sodium bicarbonate, NaHCO₃, is baking soda = A basic salt; has the capacity to deprotonate water
Hydrochloric acid, HCl = An acid
The reaction between sodium bicarbonate and hydrochloric acid is presented as follows;
NaHCO₃ + HCl → CO₂ + H₂O + NaCl
The equation for the ionic reaction is as follows;
Na⁺(aq) + HCO₃⁻(aq) + H⁺(aq) + Cl⁻(aq) → Na⁺(aq) + Cl⁻(aq) + H₂O(l) + CO₂(g)
In water, we have;
HCO₃⁻(aq) + H₂O(l) ⇄ H₂CO₃(aq) + OH⁻(aq)
The presence of a stronger solution of sodium bicarbonate, will produce more hydroxyl ions, OH⁻(aq), which will require, more HCl to neutralize
Therefore, if a stronger solution of sodium bicarbonate was used, more hydrochloric acid will be required
Part B
The solution of stronger sodium bicarbonate will contain a higher concentration of hydroxyl ions and therefore, require more HCl, to neutralize
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