Stuck on chemistry problem step by step

Question

1.00 L of a solution is prepared by dissolving 125.6 g of Naf in it. If took 180 mL of that solution and diluted it to 500 mL, determine the molarity of the resulting solution

Answer 1

In order to answer this question you first need to find out the molarity of the solution you prepared using the formula M=moles/liters. You need to convert the grams of NaF to moles which can be done by dividing the grams given by the substance's molar mass which in this case is 41.99 g/mol. Doing that division gives 2.99 moles. When plugged into the molarity equation that gives a molarity of 2.99 M. Then to figure out the resulting molarity you need to use the dilution equation (M1V1=M2V2) plugging in 2.99 for M1 and 180 for V1 since those are your initial conditions and 500 as V2 since that is your final volume while leaving the final molarity (M2) as a variable. So when plugged in the equation should be (2.99)(180)=M2(500). If you then solve for the missing variable you should get 1.08 M as the resulting solution's molarity