How many chlorides ions are present in 1.7grams of magnesium chloride crystal?
To determine the number of chloride ions present in 1.7 grams of magnesium chloride crystal, we need to know the formula of magnesium chloride first. The formula of magnesium chloride is MgCl2, which means there are two chloride ions for each magnesium ion.
The molar mass of MgCl2 is 95.21 g/mol (24.31 g/mol for magnesium and 35.45 g/mol for chlorine). Therefore, 1 mole of MgCl2 contains 2 moles of chloride ions (2 × 35.45 g/mol = 70.90 g/mol).
To calculate the number of chloride ions in 1.7 grams of MgCl2, we can use the following formula:
Number of chloride ions = (mass of MgCl2 × Avogadro's number × 2) / (molar mass of MgCl2)
where Avogadro's number = 6.022 × 10^23 mol^-1
Number of chloride ions = (1.7 g × 6.022 × 10^23 × 2) / 95.21 g/mol
Number of chloride ions = 2.23 × 10^22
Therefore, there are 2.23 × 10^22 chloride ions present in 1.7 grams of magnesium chloride crystal.