Concentrated hydrochloric acid is 38% HCl by weight and has a density of 1.19 g/mL. A...
Concentrated hydrochloric acid is 38% HCl by weight and has a density of 1.19 g/mL. A solution is prepared by measuring 36 mL of the concentrated HCI, adding it to water, and diluting to 0.500 L. Calculate the approximate molarity of this solution from the volume, percent composition, and density. Answer:
TReferencer A solution is prepared by adding 49.9 ml concentrated hydrochloric acid and 19.7 ml concentrated nitric acid to 300 ml water More water is added until the final volume is 1.00 L. Calculate H".COH)and the pH for this solution. (Hint: Concentrated HCl is 38% HCI (by mass) and has a density of 1.19 g ml., concentrated HNO, is 70% HNO, (by mass) and has a density of 1.42 g/mL.] OH")= M pH-
A solution is made by adding 42.0 mL of concentrated hydrochloric acid (37.3 wt%, density 1.19 g/mL) to some water in a volumetric flask, and then adding water to the mark to make exactly 250 mL of solution. Calculate the concentration of this solution in molarity
A certain supply of concentrated hydrochloric acid has a concentration of 36.0% HCl in water solution. The density of the solution is 1.19 g/mL. Calculate the molarity of HCl in the solution.
I. (6 pts) A certain supply of concentrated hydrochloric acid has a concentration of 40.0% HCI in water solution. The density of the solution is 1.19 g/mL. Calculate the molality and molarity of HCl in the solution. Molan Mase
Chloropropionic acid, CICH2CH2COOH is a weak monoprotic acid with Ka = 7.94 x 10-5 M. Calculate the pH at the equivalence point in a titration 48.7 mL of 0.39 M chloropropionic acid with 0.7 M KOH. Answer: Indicators of Phenolphthalein is a commonly used indicator that is colorless in the acidic form (pH < 8.3) and pink in the basic form (pH > 10.0). It is a weak acid with a pka of 8.7. What is the ratio of the...
How many milliliters of concentrated hydrochloric acid solution (36.0% HCl by mass, density = 1.18 g/mL) are required to produce 10.0 L of a solution that has a pH of 2.22?
Concentrated HCL is 37.5% by weight and has a density of 1.19g/ml. Calculate the (a) molarity of the concentrated acid (b) mL of concentrated HCL required to make 500mL of 0.2 HCl (c) ml of concentrated HCL required to make 350 ml of 0.5 N HCL
Hydrochloric acid is usually purchased in a concentrated form that is 37.0% HCl by mass and has a density of 1.20 g/mL. How much concentrated solution would you take to prepare 3.05 L of 0.545 M HCl by mixing with water?
Concentrated hydrochloric acid (HCl) (molecular mass 36.5 g/mol) has a molarity of 3.6M. What volume of concentrated HCl would you need to add to prepare a 20% (w/v) solution of HCl with a final volume of 500 mL, I have calcualted that 3.6mol/L x 36.5g/mol =131.40g/L. Then to get the 100ml value and percentage: 131.40/1000 x 100 =13.14g/100ml therefore 13.14%. 20% of this would be 2.628g. Is this the answer?