Answer:
The correct answer is 0.28 M
Explanation:
First we have to calculate the molecular weight (MM) of BaOH:
MM(BaOH) = 137.3 g/mol + 16 g/mol + 1 g/mol= 154.3 g/mol
The number of moles of BaOH there is in the solution is obtained from the mass (m) divided into the molecular weight:
moles of BaOH = m/MM(BaOH) = 4.285 g/154.3 g/mol = 0.028 moles
The molarity of the solution is the number of moles of BaOH in 1 liter of solution. So, we divide the moles into the volume and then we have to convert ml to L (1000 ml = 1 L). For this, we multiply by the conversion factor 1000 ml/1 L, as follows:
M = 0.028 moles/100.0 ml x 1000 ml/1 L = 0.28 mol/L = 0.28 M ≅ 0.3 M
Answer:
[tex]M=0.25M[/tex]
Explanation:
Hello,
In this case, molarity is defined as the relationship between the moles of the solute (barium hydroxide) and the volume of the solution in liters:
[tex]M=\frac{n_{Ba(OH)_2}}{V_{sln}}[/tex]
In this case, as the barium hydroxide molar mass is 171.34 g/mol, one obtains the molarity in molar units (M=mol/L) as:
[tex]M=\frac{4.285gBa(OH)_2*\frac{1molBa(OH)_2}{171.34gBa(OH)_2} }{100.00mL*\frac{1L}{1000mL}}\\\\M=0.25M[/tex]
Best regards.
