Molar mass of naoh

Molarity(M): • It can be defined as the number of moles of solute divided by the volume of the solution in liters. • Hence, the formula can be given as: M = n V where, n = number of moles of solute and V = volume of the solution in liters. • 10 % NaOH means 100 ml of solution containing 10 g of NaOH. • Given that, the number of NaOH solution = 10 %. The molar mass of NaOH = 40 g / mol . Thus, the number of moles 10 % NaOH = 10 40= 1 4= 0 . 25 moles Volume of 10 % NaOH solution = 100 1000 = 0 . 1 L. Molarity(M) = 0 . 25 0 . 1= 2 . 5 M. Hence, the Molarity(M) of 10 % NaOH = 2 . 5 M.

More information on molar mass and molecular weight In chemistry, the formula weight is a quantity computed by multiplying the atomic weight (in atomic mass units) of each element in a chemical formula by the number of atoms of that element present in the formula, then adding all of these products together. If the formula used in calculating molar mass is the molecular formula, the formula weight computed is the molecular weight. The percentage by weight of any atom or group of atoms in a compound can be computed by dividing the total weight of the atom (or group of atoms) in the formula by the formula weight and multiplying by 100. Using the chemical formula of the compound and the periodic table of elements, we can add up the atomic weights and calculate molecular weight of the substance. Finding molar mass starts with units of grams per mole (g/mol). When calculating molecular weight of a chemical compound, it tells us how many grams are in one mole of that substance. The formula weight is simply the weight in atomic mass units of all the atoms in a given formula. Formula weights are especially useful in determining the relative weights of reagents and products in a chemical reaction. These relative weights computed from the chemical equation are sometimes called equation weights. The atomic weights used on this site come from NIST, the National Institute of Standards and Technology. We use the most common isotopes. This is how to calculate molar mass (average molecular...

Hint: The molar mass of any compound can be calculated by adding the atomic weight of the individual atoms involved in the chemical formula of the respective chemical compound. We should know the molecular or chemical formula of the respective compound. Complete answer: - In the question it is asked to calculate the molar mass of the sodium hydroxide. - We should know the chemical formula of the sodium hydroxide to calculate the molar mass of it. - The chemical formula of the sodium hydroxide is NaOH. - We should know the atomic weights of the sodium, hydrogen and the oxygen to calculate the molar mass of the sodium hydroxide. - The atomic weight of the sodium is 23, the atomic weight of the hydrogen is 1, and the atomic weight of the oxygen is 16. - Now we can calculate the molar mass or molecular weight of the sodium hydroxide by using the formula below. Molecular weight of the NaOH = Atomic weight of the Na + Atomic weight of the H + (atomic weight of the oxygen) Molecular weight of the NaOH= 23 + 1 + (16) = 40. - Now we must express the molecular weight of the sodium hydroxide in molar mass. - The molar mass of the sodium hydroxide is 40 g/mol. Note: Without knowing the chemical or molecular formula of the compound and without knowing the atomic weights of the individual elements involved in the chemical formula it is very difficult to calculate the molar mass of the respective compound.

\( \newcommand\) • • • • • • A titration is a volumetric technique in which a solution of one reactant (the titrant) is added to a solution of a second reactant (the "analyte") until the equivalence point is reached. The equivalence point is the point at which titrant has been added in exactly the right quantity to react stoichiometrically with the analyten (when moles of titrant = moles of analyte). If either the titrant or analyte is colored, the equivalence point is evident from the disappearance of color as the reactants are consumed. Otherwise, an indicator may be added which has an "endpoint" (changes color) at the equivalence point, or the equivalence point may be determined from a titration curve. The amount of added titrant is determined from its concentration and volume: n (mol ) = C (mol /L) * V (L) and the amount of titrant can be used in the usual stoichiometric calculation to determine the amount of analyte. The titration process can be observed in the video below. A measured volume of the solution to be titrated, in this case, colorless aqueous acetic acid, CH 3COOH( aq) is placed in a beaker. The colorless sodium hydroxide NaOH( aq), which is the titrant, is added carefully by means of a buret. The volume of titrant added can then be determined by reading the level of liquid in the buret before and after titration. This reading can usually be estimated to the nearest hundredth of a milliliter, so precise additions of titrant can be made rapidly. Figure \(\P...

You can go from moles of sodium hydroxide, #"NaOH"#, to grams of sodium hydroxide by using a conversion factor called molar mass. The molar mass tells you the mass of exactly one mole of a given substance. In this case, sodium hydroxide has a molar mass of #"39.997 g mol"^(-1)#, which implies that one mole of sodium hydroxide has a mass of #"39.997 g"#. You can thus use the molar mass of sodium hydroxide to calculate how many grams you'd get in #0.25# moles of this compound #0.25 color(red)(cancel(color(black)("moles NaOH"))) * "39.997 g"/(1color(red)(cancel(color(black)("mole NaOH")))) = color(green)(|bar(ul(color(white)(a/a)color(black)("10. g")color(white)(a/a)|)))# The answer is rounded to two

\( \newcommand\) • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • Objectives • To perform an analytical titration. • To standardize a basic solution. • To determine the molecular mass of an unknown acid. Chemical reactions between acids and bases are important processes. These reactions can be used to synthesize new substances or to analyze the quantity of a pure substance or of a compound in a mixture. In this experiment, you will first determine the concentration of a base, NaOH, and then use this standardized base to determine the molar mass of an unknown weak acid. Based on the molar mass you will determine the identity of the unknown weak acid. In water strong acids produce hydronium ions and strong bases produce hydroxide ions. The reaction of a strong acid with a strong base is represented with the chemical reaction shown in Equation1. Chemists regard this as a reaction that goes to completion; that is all of the reactants are converted to products. \[\ce\] The method of analysis will be a titration of acid with base. In the first part of the experiment, you will standardize (determine the exact concentration of) your sodium hydroxide solution. We will determine the concentration of the solution by titrating a known mass of a known acid with your sodium hydroxide solution, using an acid-base indicator to find the endpoint of the titration. In the second part of the experiment, we will determine the identity of an acid by titrating a know...