Calculate the concentration of all ions present in each of the following solutions of strong electrolytes. a. 0.300 mole of Ca (NO3), in 300.0 mL of solution M MNO,- M b. 4.5 moles of Na2 SO4 in 1.25 L of solution MNa+ Mso,- м c. 8.60 g of NH4 Cl in 100.0 mL of solution MNH,* M + = Mcr M

B. How many milliliters of 9.95 M hydrochloric acid solution should be used to prepare 4.00 L of 0.300 M HCl? C. Calculate the number of milliters of 0.764 M NaOH required to precipitate as AgOH all of the Ag+ ions in 167 mL of 0.632M AgNO3 solution. D. An aqueous solution of hydrobromic acid is standardized by titration with a 0.169 M solution of barium hydroxide.If 13.0 mL of base are required to neutralize 13.0 mL of the acid, what is the molarity of the hydrobromic acid solution? E. Oxalic acid dihydrate is a solid, diprotic acid that can be used in the laboratory as a primary standard. Its formula is H2C2O4•2H2O.A student dissolves 0.631 grams of H2C2O4•2H2O in water and titrates the resulting solution with a solution of sodium hydroxide of unknown concentration. If 24.1 mL of the sodium hydroxide solution are required to neutralize the acid, what is the molarity of the sodium hydroxide solution ? F. The concentration of Cu+ in a solution is determined by titrating it with a…

1. If 10. g of AgNO3 is available, what volume of 0.40 M AgNO3 solution can be prepared? Volume =   mL? 2. A 7.52-g sample of a diprotic acid requires 179.0 mL of a 0.750 M NaOH solution for complete neutralization. Determine the molar mass of the acid.  g/mol?

Indicate the concentration of each ion present in the solution formed by mixing 3.60 grams of KCl in 75 mL of 0.250 M cacl2 solution. Assume that the volumes are additive.

Gg.168.

6. Acid/base titration is a common method to determine the molarities of acids or bases, the molarity of certain salts can also be determined by titration. It took 22.34 mL of 0.5861 M HCl solution to neutralize 25.00 mL NaNO₂ solution. The acid- dissociation constant of HNO₂ is 4.511 × 10-¹. NaNO₂ + HCl → HNO₂ + NaCl Please answer the following questions. A What is pH of the NaNO₂ solution before titration? Hint, calculate the molarity of the NaNO₂ solution first. pH = Please provider your answer below. ( Check answer 7²² B. M HCl solution was added to the NaNO2 solution? pH = 00 0 Please provider your answer below. What is the pH when 12.78 mL of 0.5861 (0) Check answer C. What is the pH when 14.39 mL of 0.5861 M HCl solution was added to the NaNO₂ solution AFTER the equivalence point? pH = Please provider your answer below. 00 0 °C? pH= Please provider your answer below. Check answer What is the pH at equivalence point at 25 A → ← Check answer ← $ H $

Consider the neutralization reaction 2 HNO, (aq) + Ba(ОН), (аq) — 2 Н, О() + Ва(NO,), (aq) A 0.120 L sample of an unknown HNO, solution required 30.1 mL of 0.250 M Ba(OH), for complete neutralization. What is the concentration of the HNO3 solution? concentration: M

A student is asked to standardize a solution of sodium hydroxide. He weighs out 1.09 g potassium hydrogen phthalate (KHC8H404, treat this as a monoprotic acid). It requires 33.5 mL of sodium hydroxide to reach the endpoint. Use the References to access important values if needed for this question. A. What is the molarity of the sodium hydroxide solution? This sodium hydroxide solution is then used to titrate an unknown solution of nitric acid. Submit Answer M B. If 18.7 mL of the sodium hydroxide solution is required to neutralize 10.3 mL of nitric acid, what is the molarity of the nitric acid solution? 2 question attempts remaining M