
What is the of the resulting solution when equal volumes of and are mixed ?
A.
B.
C.
D.
Answer
510k+ views
Hint: To calculate first of all we have to find concentration of ion also and to calculate we have to calculate concentration of ion in the resulting solution . We should remember the formula .
Complete step by step answer:
Chemical reaction for the given solution is : .
Let us assume volume of both and is equal to then we have moles of and moles of by using the formula where is number of moles , is molarity and is volume of the solution .
Since we have mole of and only mole of , so only mole of ion will take part in neutralisation reaction .
Now number of moles of ion
Total volume of solution
Concentration of
Now we know that . So of the resulting solution will be equal to .
So option (C) is the correct answer .
Note:
High means that the solution is basic in nature as it is clear from the above question because it has an excess amount of and its value is greater than seven . Similarly the high value of means solution is acidic in nature . Neutral solutions have both and of seven . Another point to be noted down is that decreases with increase in temperature because as the temperature rises molecular vibrations increases which results in the ability of water to ionise and form more hydrogen ions . As a result will drop . But we should not be confused that water becomes more acidic at a higher temperature because a solution is considered to be acidic if there is excess hydrogen ions . In the case of water there is always the same concentration of and .
Complete step by step answer:
Chemical reaction for the given solution is : .
Let us assume volume of both
Since we have
Now number of moles of
Total volume of solution
Concentration of
Now we know that
So option (C) is the correct answer .
Note:
High
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