When a 5.00-g sample of rbbr is dissolved in water in a calorimeter?
1 answer:
To answer this question, I found a similar problem as shown in the picture below. Let's use the given information: Heat capacity = 3.565 kJ/K, ΔT = 0.26 K. Also, the molar mass of RbBr is 165.372 g/mol.
The solution is as follows:
Molar Heat of Solution = (3.565 kJ/K)(0.26 K)(1/ 5 g)(165.372 g/mol)
<em>Molar Heat of Solution = 30.66 kJ/mol</em>
The solution is as follows:
Molar Heat of Solution = (3.565 kJ/K)(0.26 K)(1/ 5 g)(165.372 g/mol)
<em>Molar Heat of Solution = 30.66 kJ/mol</em>
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Answer:
0.007 M
Explanation:
pH is defined as the negative logarithm of the concentration of hydrogen ions.
Thus,
pH = - log [H⁺]
The expression of the pH of the calculation of weak acid is:-
Where, C is the concentration = ?
Given, pH = 3.45
So, for ,
C = 0.007 M