Achemist prepares a solution of magnesium fluoride (mgf_2), by measuring out 0.031 g of magnesium fluoride into a 250. ml. volumetric flask and filling the flask to the mark with water. calculate the concentration in mol/l of the chemist magnesium fluoride solution. round your answer to 2 significant digits. mol/l.

The concentration of the magnesium fluoride solution is 0.0020 M

Explanation:

Step 1: Data given

Mass of MgF2 = 0.031 grams

volume = 250 mL = 0.250 L

Molar mass of MgF2 = 62.3 g/mol

Step 2: Calculate moles

Moles MgF2 = mass MgF2 / molar mass MgF2

Moles MgF2 = 0.031 grams / 62.3 g/mol

Moles MgF2 = 4.98 *10^-4 moles

Step 3: Calculate concentration of MgF2

Concentration MgF2 = moles MgF2 / volume

Concentration MgF2 = 4.98 *10^-4 / 0.250 L

Concentration = 0.0020 M

The concentration of the magnesium fluoride solution is 0.0020 M

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the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.