If a student mixes 75 mL of 1.30 M HNO3 and 150 mL of 6.5 M NaOH. is the final solution acidic, basic, or neutral
1 answer:
Answer:
The solution is basic.
Explanation:
We can determine the nature of the solution via determining which has the large no. of millimoles (acid or base):
If no. of millimoles of acid > that of base; the solution is acidic. If no. of millimoles of acid = that of base; the solution is neutral. If no. of millimoles of acid < that of base; the solution is basic.
We need to calculate the no. of millimoles of acid and base: no. of millimoles of acid (HNO₃) = MV = (1.3 M)(75.0 mL) = 97.5 mmol.
no. of millimoles of base (NaOH) = MV = (6.5 M)(150.0 mL) = 975.0 mmol.
<em>∴ The no. of millimoles of base (NaOH) is larger by 10 times than the acid (HNO₃). </em>
<em>So, the solution is: basic. </em>
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Answer:
C. from y to z
Explanation:
HCL 2.0x 3.6790= KOH SOLITION
<span>(8.5 x 10^-3 mol) / (0.0320 mol/L KCN)=0.265625 L=265.625 ml.
This is the volume of a 0.0320 M KCN solution that would give a median lethal dose to a 185 lb person.</span>
C2H2O4 C2HO4- + H+
0.175 - x x x + y
C2HO4- c2o42– + H+
x - y y x + y
K2 = (y) (x +y) / (x-y)
As, y << x
So, K2 = (y) (x) / (x)
K2 = y =6.1 × 10^–5
Hence, concentration of (c2o42–) 6.1 × 10^–5 M
The answer is C.) hoped this helps
