To solve this question, we need to determine key pieces of information for the neutralization reaction between the acid solution (HX) and the base solution (Na₂CO₃). Here is the step-by-step solution:
1. Determine the concentration of the acid HX solution (A):
The concentration of the acid HX is given as 3.5 g/dm³.
2. Calculate the total volume of the base solution (B):
We are given the average volume of the base solution required for neutralization: 26.10 cm³ + 0.25 cm³ = 26.35 cm³.
3. Convert the volume of the base solution from cm³ to dm³:
- [tex]\( 1 \text{ dm}^3 = 1000 \text{ cm}^3 \)[/tex]
Therefore, [tex]\( 26.35 \text{ cm}^3 = \frac{26.35}{1000} \text{ dm}^3 = 0.02635 \text{ dm}^3 \)[/tex].
4. Determine the number of moles of the acid HX in the solution:
The concentration of the acid HX is given in g/dm³ and we want to find the number of moles. Assuming the molecular weight is implicitly known but not directly needed (because of the mole ratio understanding), we treat this straightforwardly in the reaction.
5. Calculate the moles of acid HX in 1 dm³ of solution:
- Given 3.5 grams of HX in 1 dm³, we can relate it to the concentration directly for neutrality checking which often assumes mole equivalence or a simple mole ratio.
- [tex]\( 3.5 \text{ g} = 0.0035 \text{ moles of HX in 1 dm}^3 \)[/tex].
6. Determine the moles of Na₂CO₃ needed for neutralization:
Assuming a simple 1:1 mole ratio for neutralization for simplicity (unless exact stoichiometric coefficients of HX to Na₂CO₃ given), the moles of Na₂CO₃ will match the mole number derived from HX use:
- [tex]\( \text{Moles of Na}_2\text{CO}_3 = 0.0035 \times 0.02635 = 9.2225 \times 10^{-5} \text{ moles} \)[/tex].
To summarize, we found the required numbers for neutralization:
- Concentration of Acid (HX): 3.5 g/dm³.
- Total Volume of Base Solution (B): 26.35 cm³.
- Volume of Base in dm³: 0.02635 dm³.
- Moles of acid HX used: 0.0035 moles per dm³.
- Moles of base (Na₂CO₃) involved: 9.2225 x 10⁻⁵ moles.
Therefore, in the neutralization reaction between the given acid and base, these computed numbers represent the quantities and mole figures correctly involved.
