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How many mL of concentrated HCL solution are needed to provide 90.0g of HCL? Concentrated HCL solution is 37.0% HCl by weight and has a density of 1.19 g/mL.

Md Ariful Islam

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Md Ariful Islam

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p =m/V 1,19 = 90/V V = 75,63 ml - it's volume of 37% HCL Need to solve a mass of full solution ( x = V(HCL)+(H2O) ), then 75,63 ml - 37% x - 100%. x = 75,63x100/37 = 204,4 ml (volume of 37% concentrated HCL).
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Determine the types of products produced at each electrode if the solution is made of A. Concentrated NaF B. Diluted NaF C. Concentrated CaO D. Diluted CaO E. Diluted Na2S F. Concentrated Na2S

A. Anode: F2; Cathode: NaB. Anode: O2; Cathode: H2C. Anode: O2; Cathode: CaD. Anode: O2; Cathode: H2E. Anode: S; Cathode: H2F. Anode: S; Cathode: Na

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A concentrated solution of HCl has a molarity of 10.0 M. You add 23.50 mL to a flask and then dilute with water. The mass of the final solution is 125.0 g. What is the mass percent of HCl ?

Mass percent essentially means g of HCl/total grams of solution (x100%). So, in this problem we already know the total mass = 125.0 g. If we can find the mass...

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A sample of concentrated HCl solution with 88% by mass and density of 1.43 g cm⁻³. Calculate the molality of the solution

HCl solution with 88% means 100g of Solution contains 88g of HCl Moles of HCl = 88g/(36.45g/mol) = 2.41 molDensity of solution = 1.43 gcm-3 = 1.43g/mL 100g...

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Concentrated Hydrochloric acid is commonly sold as 12.0 M HCL and its density is 1.18 g/cm^3 . Calculate: (a)the Molality of the solution. (b) the weight percent of HCL in the solution

The molality, b, of a solution is the amount of substance (in mol) of solute, divided by the mass (in kg) of the solvent (not the mass of the solution):...

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describe the preparation of 100ml of 0.1 M HCl from a concentrated solution that has a specific gravity of 1.18 and is 37%(w/w) HCl ?

(1000 mL/ 1L)(1.18 g/mL) · (0.37) · (1mol HCl/36.5 g HCl) = 11.96 M We want to make 100 mL of 0.1 M: 100 mmol HCl required V x M...

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A concentrated HCl solution contains 37% w/w HCl. The specific gravity of the solution is 1.19 g/mL. Calculate its molarity

CM=n/V100 g of a given solution has a volume of:V (HCl) = 100/1.19 = 84.03 mln = m/MM (HCl) = 36.5 mol/ln (HCl) = 37/36.5 = 1.01 molCM (HCl) =...

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6.) A 11.5 ml solution of HCl has 0.531 g/L of HCl in solution. Calculate the concentration, amount of moles of HCl, and pH of the solution.

1)C(HCl)=0.531/36.5=0.0145 mol/L2)n(HCl)=0.531*0.0115/36.5=1.673 *10^-4 mol3)pH=-lg[H+]=-lg(1.673*10^-4)=3.78

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A 11.5 ml solution of HCl has 0.531 g/L of HCl in solution. Calculate the concentration, amount of moles of HCl, and pH of the solution

0.0115 x 0.531/36.5 = 1.67e-4 moles.1.67e-4/0.0115=0.0145 M.pH: 1.83863199777

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34.62 mL of a 0.3 M Mg(OH)2 solution are needed to neutralize a 15-mL solution of HCl on unknown concentration. Calculate the concentration of HCl solution.

Mg(OH)2+2HCl=MgCl2+2H2O1.Trace by finding the amount of Mg(OH)2. To do this, we multiply the molarity by the volume (liters): 0.03462litres *0.3 mol/litres= 0.010386 mol Mg(OH)22.based on the reaction we find the amount...

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What volume of 17.8 M sulphuric acid solution would be needed to make 2.00 L of 0.200 M solution by dilution of the original, concentrated stock solution?

Proportion 1:0.2 mol – 1 Lx mol – 2 Lx = 0.4 mol is needed to make the new solutionsProportion 2:17.8 mol – 1 L0.4 mol – yy = 0.0225...

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