more volume of NaOH means more moles of NaOH (volume * molarity = mole ; molarity=constant) , more moles of NaOH means more grams and mole of HCl and more grams and/or mole and/mass of M2CO3 (note that they are both on the same side of the reaction)
now note that if the mass of M2CO3 is known and u want to calculate the molar mass of it, since mass / mole = molar mass, so the molar mass will be smaller than the real one . . but if the mole are known and you want to calculate the molar mass again since mass/molar = molar mass, this time the calculatod moalr mass will be higher then the actual one
I don't see a question in all of this. Frankly, it's confusing, too.
I understand that you're discussing the relationship between the volume of NaOH, the number of moles of NaOH, and the resulting amounts of substances involved in a chemical reaction. You also mentioned calculating the molar mass of a compound using either known mass or known moles. Allow me to explain further:
1. Volume of NaOH and moles of NaOH: When you have a solution of NaOH, the volume multiplied by the molarity gives you the number of moles of NaOH. This relationship is expressed using the equation volume * molarity = moles. Therefore, increasing the volume of NaOH will result in more moles of NaOH.
2. Moles of NaOH and amounts of substances: In a chemical reaction involving NaOH, the number of moles of NaOH influences the amounts of other substances participating in the reaction. If the reaction involves HCl and M2CO3, an increase in the moles of NaOH will lead to an increase in the moles of HCl and M2CO3 on the same side of the reaction. More moles of these substances generally mean more grams or more moles/mass of M2CO3.
3. Molar mass calculation using mass: If you know the mass of M2CO3 and want to calculate its molar mass, you can use the equation mass/moles = molar mass. However, it's important to note that this calculated molar mass will be smaller than the actual molar mass of M2CO3 since the mass is known and the calculated moles will be higher due to the volume of NaOH and the resulting moles of HCl and M2CO3.
4. Molar mass calculation using moles: Conversely, if you already know the moles of M2CO3 and want to calculate its molar mass, the equation mass/molar mass = moles can be used. In this case, the calculated molar mass will be higher than the actual molar mass since the moles are known, and the calculated mass will be affected by the increased volume of NaOH and the resulting moles of HCl and M2CO3.
It's important to keep in mind that these calculations depend on the specific reaction and the stoichiometry involved. The reaction coefficients and the balanced equation are crucial in determining the relationships between volume, moles, and masses of the substances involved.