Well, look at the definitions of each quantity.... "Molarity"="Moles of solute"/"Volume of solution" "Molality"="Moles of solute"/"Kilograms of solvent" "Molality" is thus independent of temperature, whereas "molarity" changes slightly with temperature as the density of the solution changes. For dilute solutions, "molarity"-="molality". to a very good approximation.
Moles n solution: Calculate the molarity of a solution of NaOH made by dissolving 2moles of sodium hydroxide in water and making up to 250cm^3?
Moles n solution: Calculate the molarity of a solution of ... - Socratic
What is the molarity of 156 mL of solution made from 2.5 grams of KCl?
What is the molarity of 156 mL of solution made from 2.5 ... - Socratic
Titration affects molarity by changing the volume of the solution. For example, if you have a 1M solution of NaOH in 1 Liter, then you have 1M Na+ ions. If you titrate this with 1M HCl, then it will take 1 Liter of HCl to fully titrate this. However, your Na+ ion concentration is now 1 mole in 2 liters, or 0.5M. So titrations generally increase volume and reduce molarities
Every time you're looking for a solution's molarity, you must determine how many moles of solute you get in one liter of solution. That is what molarity essentially tells you - how many moles of solute you'd get if you had exactly one liter of solution. ∣∣ ∣ ∣ ∣ ...
What is the molarity of a solution prepared by dissolving 2.350 g KI in enough water to make 175.0 mL of solution ?