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35 mL of 0.1 M solution is used to neutralize 25 mL of barium hydroxide. The molarity of Barium hydroxide solution is
- a)0.28
- b)0.07M
- c)0.14M
- d)0.35
Correct answer is option 'B'. Can you explain this answer?
Most Upvoted Answer
35 mL of 0.1 M solution is used to neutralize 25 mL of barium hydroxid...
Yes option B is correct... here is the brief solution nikhil...as per your request on my last update of answer to u this qn.. Solution; 1st right the equation; Ba(OH)2+2HCl----->BaCl2+2H2O and the formula is ; M1×V1÷n1=M2×V2÷n2 where; ( M1 and M2 are the molarity of Ba(OH)2 and HCl and V1 and V2 are the volume of Ba(OH)2 and HCl and n1 and n2 are the stochiometric coefficients...) so; as per question; given data; (M2=35 and V2=0.1 and n2=2 and V1=25 and n1=1 and M1=?....) substitute the values; M1=M2×V2×n1÷n2×V2 M1=35×0.1×1÷2×25 M1=3.5÷50 so; molarity of barium hydroxide is 0.07 moles...i hope u will understand my answer now..👍!reply me if u r understand...😊
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35 mL of 0.1 M solution is used to neutralize 25 mL of barium hydroxid...
Calculation of molarity of Barium hydroxide solution
Given:
Volume of acid solution (V1) = 35 mL
Molarity of acid solution (M1) = 0.1 M
Volume of base solution (V2) = 25 mL
Molarity of base solution (M2) = ?
To calculate the molarity of Barium hydroxide solution, we will use the formula:
M1V1 = M2V2
Substituting the values in the formula, we get:
0.1 x 35 = M2 x 25
M2 = (0.1 x 35) / 25
M2 = 0.14 M
Therefore, the molarity of Barium hydroxide solution is 0.14 M. Option B is the correct answer.
Note: In a neutralization reaction, the moles of acid and base are equal. So, we can use the formula M1V1 = M2V2 to calculate the molarity of either acid or base, provided we know the molarity and volume of the other.
Given:
Volume of acid solution (V1) = 35 mL
Molarity of acid solution (M1) = 0.1 M
Volume of base solution (V2) = 25 mL
Molarity of base solution (M2) = ?
To calculate the molarity of Barium hydroxide solution, we will use the formula:
M1V1 = M2V2
Substituting the values in the formula, we get:
0.1 x 35 = M2 x 25
M2 = (0.1 x 35) / 25
M2 = 0.14 M
Therefore, the molarity of Barium hydroxide solution is 0.14 M. Option B is the correct answer.
Note: In a neutralization reaction, the moles of acid and base are equal. So, we can use the formula M1V1 = M2V2 to calculate the molarity of either acid or base, provided we know the molarity and volume of the other.
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35 mL of 0.1 M solution is used to neutralize 25 mL of barium hydroxide. The molarity of Barium hydroxide solution isa)0.28b)0.07Mc)0.14Md)0.35Correct answer is option 'B'. Can you explain this answer?
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