Answer:
Explanation:
Hello,
In this case, since in a dilution process the moles of the solute must remain unchanged, we use the volumes and molarities as shown below:
Clearly, the concentrated solution is 12M and the diluted solution is 0.5 M, thus, the volume of the concentrated solution we should take is:
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<span>The atomic mass for copper is 63.546 amu. Copper is typically reddish orange in color and has a melting point of 1981.4 degrees Fahrenheit. It is classified as a transition metal and has an atomic number of 29.</span>
1. For the first question, we must find the mass of the anhydrous salt, MgSO₄. The molar mass for MgSO₄·7H₂O is 246.47 g/mol, while that of MgSO₄ is 120.37 g/mol.
7.834 g MgSO₄·7H₂O * 1 mol MgSO₄·7H₂O/246.47 g * 1 mol MgSO₄/1 mol MgSO₄·7H₂O * 20.37 g MgSO₄/mol = <em>0.647 g MgSO₄</em>
2. Mass of Water = Mass of sample - Mass of anhydrous sale
Mass of water = 7.834 - 0.647 = 7.19 g
Percent Water in Hydrate = 7.19/7.834 * 100 = <em>91.74%</em>
Explanation:
Molarity = M = mol/1 liter
in sol 250 mL there are KNO3 2.02 mol
in sol 1000 mL there are KNO3 = 2.02/250 × 1000
= 8.08 mol/liter
Answer:
0.1 M NaCl
Explanation:
This question reminds of of the solubility rules. Let us recall that all chlorides are soluble except those of lead, mercury II and silver which are insoluble in water.
The following reaction will occur leading to the formation of a precipitate;
Pb(NO3)2(aq) + 2NaCl(aq) -------> 2NaNO3(aq) + PbCl2(s)
The white precipitate formed is PbCl2.
