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Commercial hydrochloric acid is available as a 10.17 molar solution. How would you use this to...
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-
How could you make 2.5 L of 0.10 M hydrochloric acid? Question 10 (1 point) How could you make 2.5 L of 0.10 M hydrochloric acid? Hint: This is a dilution. How many moles of HCI in 2.5L of 0.1M? Use the fact that M = ? that M - n moles so # of moles n = M, V =.. O dilute 59.4 mL of 3.0 M HCl to 2.5 L with water O dilute 0.25 L of pure...
4 June 2019 CHEM 177-Su19 Chapter 4 APP-1 4. Hydrochloric acid (HCI) is generally sold as an 11.65 M solution. When doing titration experiments, many will use an HCl concentration of 1.00 M HCl. If you wanted to make 150 mL of 1.00 M HCI, how many mL of the stock HCl solution would you need? 5. A 4.00 L stock solution of H3PO4 of unknown concentration was mixed with 4.00 L of pure water. The concentration of the new...
How much of a 21.0 M hydrochloric acid solution would you dilute to prepare 50.00 mL of 9.00 M HCl?
The Na,Co, solution described above was used to analyse a hydrochloric acid solution of unknown concentration. It was found that 24.30 mL of the Na,Co, solution was required to neutralise a 20.00 mL sample of the hydrochloric acid solution. 4. Using your answer to part 3 above, calculate the amount of Na,Co, present in 24.30 mL of the Na,Co, solution. (2 marks) 5. Using your answer to part 2 above, deduce the amount of HCl that was present in the...
Commercial hydrochloric acid is 12.4 M. A chemist wants to prepare 0.334 M HCI. How many milliliters (ml) of the acid is required to make up 1.75 L of the dilute acid? 1 decimal place, fill in the number ONLY.
(10 pts) A solution is prepared by dissolving 1.239 grams of hydrochloric acid, HCI, in enough water to make 250.0 mL of solution. A 25.00 mL sample of this solution is diluted with water to a final volume of 100.0 mL. Now, you take 10.00 mL of that solution and dilute it to 100.00 mL What is the molarity of the final solution? (HCI 36.45 g/mol)
Click to see additional instructions The molar heat of neutralization from hydrochloric acid (HCI) and sodium hydroxide (NaOH) is -56.1 kJ/mol. Use this accepted value to predict that heat evolved during the neutralization of 168 mL of 3.00 M HCl solution with 168mL of 3.00 M NaOH solution KJ
ANAL 425: Titrating Hydrochloric Acid Solution with a Standard Sodium Hydroxide Solution ANAL 42: The Hydrochlork Acil Solution with Standard Sodium Hydroxide Solution (3) Calculate the number of equivalents of acid in 1.00 lb of dry acid powder. The molar mass of NaHSO, is 120.07 g mol (4) Calculate the mass, in pounds, of dry acid powder required to supply the equivalent amount of acid present in 1 qt (0.9463 L) of the commercial muri- atic acid solution discussed in...
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: