6M
Molarity is defined by amount of solute per unit volume; the density is irrelevant; therefore, the molar is simply 0.142 as stated in the question.
molarity = mol / litre The concentration is 10% HCl in water, assuming this is expressed in w/v (weight to volume) as this is the normal way. The density of 10% HCl is unknown but will be estimated to be the same as water (although slightly incorrect), since no data is given. 1 L of which 10% are HCl is assumed to weigh 1000 grams. 10% HCl x 1000g = 100g of HCl. 100g of HCl is present in 1 L. The mw of HCl = 36.5g/mol, 100g/(36.5g/mol) = 2.74mol is present in 1 L. The molarity is 2.74mol / 1 L = 2.7 M (two significant figures) (Looking up hydrochloric acid in wikipedia tells us that the density of a 10% solution is actually 1048g/L and the actual molarity becomes 2.87M. The calculated number was close enough, but it shows that the density is important. Molality on the other hand is mol/kg, so with molality we can skip the unknown density problem. For practical purposes, molarity is still the mostly used one, because volume is easier to measure than weight in the laboratory when handling toxic solvents that are unhealthy to inhale.)
Molarity =(% by weight x density x 1000 mL/litre)/(Molecular weight x 100%) %by weight ={(Molarity x Molecular Weight)/(density x 1000 mL/litre)} x 100% Molecular weight - grams/mol (36.461 g/mol for HCl) Molarity - mol/litre Density - g/millilitre (Density may be listed as specific gravity) For the given conditions Conc.HCl 37.0%, sp.gr. 1.19 Molarity = (37.0 x 1.19 x 1000)/(36.461 x 100) Molarity = 12.07592 M Available = 12.07592 M HCl Required = 0.300 M HCl: V1 x C1 = V2 x C2 (1000[mL] x 0.300[M]) / (12.07592[M]) = 24.84283[mL] Dilute 24.84mL of 37.0% HCl to one liter to get 0.300M HCl solution.
17 M
If the density is 1.0 g/ml, one liter of the solution will weigh 1000 grams. 3.0 % of this mass or 30 grams of it is constituted of H2O2. The molar mass of H2O2 is 2 (1.008 + 15.999) = 34.014. The molarity of this solution is therefore 30/34.014 = 0.88, to the justified number of significant digits.
Increasing the amount of the solute in the solution the molarity and the density of this solution increases.
Not enough information. To calculate mass, you would need volume and density (mass = volume x density).
Density is the weight per volume of a solution, while the concentration is the amount of particles/molarity per volume.
Is the makeup of the solution expressed as "percent by mass"? If so, to calculate molarity (or normality), you have to also know the density of the solution Step 1. Lets say the solution is 14%, and the density is 1.09 g/mL. We can write the following: (14 grams solute/100 grams solution) (1.09 grams solution/ mL solution) Step 2. Multiplying and cancelling from step 1 gives you 15.26 grams solute / 100 mL solution. Multiplying top and bottom by 10 gives you 152.6 grams solute per liter. Step 3. Molarity is number of moles per liter. Divide the 152.6 grams of the solute by the forumua weight (or molecular weight) of the solute, and you have the number of moles of solute. This number is therefore the molarity of the solution. If the solution is "percent by volume", the number you have is number of grams per 100 mL. Multiply by 10, and you have grams per liter. Then divide by the formula weight, and you have the molarity.
1.12 m
Molarity is the no of moles of solute dissolved per litre of a solution. now if u want to find it from the percentage purity , here is the formula for that Molarity = % purity x density x 10 ___________________ molar weight of the solute note : density is usually given %purity problems, if its not u can evualvate it from from formula { d= mass/volume} i hope it solves the problem
Molarity is defined by amount of solute per unit volume; the density is irrelevant; therefore, the molar is simply 0.142 as stated in the question.
0.736 i think good luck
molarity of moles of solute/liters of solution(not solvent) the volume of the solvent(even if it started at 1 L) would change after adding the solute depending on the molar mass, density, etc of the solute, the molarity would be different
The concentration is 1 mol/L or 5,611 g KOH/100 mL solution.
In dilute solutions... ie closer a solution is to pure water the closer molality and molarity come to equalling each other. This is because the molality uses mass and molarity uses volume, the ratio of these two (mass and volume) is density, and water has the density of 1 therefore the mass and volume are equal to each other. THEREFORE calculating the molarity of water is the same as calculating the molality of water.
6 kg = 6000 grams and density of water = 1.00 grams/milliliters. 1.00 g/ml = 6000 grams/X ml = 6000 ml which = 6 liters ======================== Molarity = moles of solute/Liters of solution Molarity = 2 moles NaOH/6 Liters = 0.3 M NaOH solution -----------------------------