when 12.5mL of 0.28M HNO3 and 5.0mL OF 0.46M Ba(OH)2 are mixed, is the resulting solution acidic, basic, or neutral?
2HNO3 + Ba(OH)2 ==> 2H2O + Ba(NO3)2
moles HNO3 = M x L = ??
moles Ba(OH)2 = M x L = ??
Convert moles HNO3 and Ba(OH)2 to moles of the product and the SMALLER answer is the one to choose. The reactant left over is what determines the final pH.
To determine the acidity or basicity of the resulting solution after mixing HNO3 and Ba(OH)2, we need to analyze the reaction between these two compounds.
The balanced chemical equation for the reaction is as follows:
HNO3 + Ba(OH)2 → Ba(NO3)2 + H2O
From the equation, you can see that HNO3 and Ba(OH)2 react to form Ba(NO3)2 and water (H2O).
Now, let's calculate the moles of HNO3 and Ba(OH)2 used in the reaction:
Moles of HNO3 = volume (in L) × concentration (in M)
= 12.5 mL × (1 L / 1000 mL) × 0.28 M
= 0.0035 moles
Moles of Ba(OH)2 = volume (in L) × concentration (in M)
= 5.0 mL × (1 L / 1000 mL) × 0.46 M
= 0.0023 moles
Looking at the balanced equation, we can see that the stoichiometric ratio between HNO3 and Ba(OH)2 is 1:1. This means that for every 1 mole of HNO3 used, 1 mole of Ba(OH)2 is also used.
Comparing the moles of these two compounds, we can see that the moles of HNO3 (0.0035 moles) are greater than the moles of Ba(OH)2 (0.0023 moles). This implies that there is an excess of HNO3 in the reaction.
Since HNO3 is a strong acid and Ba(OH)2 is a strong base, the excess of HNO3 will determine the nature of the resulting solution.
Having an excess of HNO3 means that there are still some HNO3 molecules left in the solution after the reaction. Since HNO3 is an acid, the excess HNO3 will make the resulting solution acidic.
Therefore, the resulting solution is acidic.