Concept explainers
For each of the following solutions, calculate the:
a.liters of a
b. liters of a
c. milliliters of a
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Basic Chemistry
- Calculate the mass of potassium cyanide ion that must be added to 100 mL of solution to dissolve 2.0102 mol of silver cyanide, AgCN.arrow_forwardA 1.00 liter solution contains 0.45 M hydrocyanic acid and 0.58 M sodium cyanide. If 0.15 moles of barium hydroxide are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of barium hydroxide.) A. The number of moles of HCN will decrease. B. The number of moles of CN will remain the same. BC. The equilibrium concentration of H3O+ will remain the same. D. The pH will remain the same. E. The ratio of [HCN] [CN] will increase.arrow_forward1. How do you prepare a 100mL of 0.1 M phosphate buffer?To make 100 mL of 0.1 M phosphate buffer: Calculate the amount of sodium phosphate needed. moles of sodium phosphate = (0.1 mol/L) x (0.1 L) = 0.01 moles mass of sodium phosphate = moles x molar mass = 0.01 moles x 142 g/mol = 1.42 g Dissolve 1.42 g of sodium phosphate in distilled water in a 100 mL volumetric flask. Adjust the pH of the solution to the desired value (usually around 7.4) using a strong acid or strong base. Bring the solution to the final volume (100 mL) with distilled water. 2. From the anterior buffer, how do you make 100mL of 0.05 M? To make 100 mL of 0.05 M phosphate buffer from the 0.1 M stock solution: Calculate the amount of the 0.1 M phosphate buffer needed. moles of phosphate buffer = (0.05 mol/L) x (0.1 L) = 0.005 moles Calculate the volume of the 0.1 M phosphate buffer needed. moles = concentration x volume (in liters) volume = moles / concentration = 0.005 moles / 0.1 mol/L = 0.05 L or 50 mL Measure…arrow_forward
- A flask contains 0.015 mol of HCl in 10.0mL of solution. a. What is the molarity of the HCl solution? b. In a titration with NaOH, how many moles of NaOH will be required to reach the end point? c. If 12.5 mL of NaOH are required to reach the end point, what is the molarity of the NaOH solution?arrow_forward5. Use YOUR stock of 0.50 M sodium acetate and your stock of 0.50 M acetic acid to make each of the solutions below: Note: You can just give your graduated cylinder (and any other glassware) a quick rinse with tap water and deionized water between making each of these solutions. Since they are variations on the same idea you don't need to wash with soap and water between uses. a. Buffer A: 100 mls of a solution of 0.010 M acetic acid and 0.090 M sodium acetate i. What volume of stock acetic acid will you use to make this solution? ii. What volume of stock sodium acetate will you use to make this solution? iii. If I had wanted to, I could have given you the directions for making buffer A in terms of dilution factors. In that case what would be the dilution factor for the acetic acid?arrow_forwardA 1.00 liter solution contains 0.35 M ammonia and 0.27 M ammonium bromide.If 0.13 moles of perchloric acid are added to this system,indicate whether the following statements are true or false.(Assume that the volume does not change upon the addition of perchloric acid.) A. The number of moles of NH3 will decrease. B. The number of moles of NH4+ will remain the same. C. The equilibrium concentration of H3O+ will increase. D. The pH will decrease. E. The ratio of [NH3] / [NH4+] will increase.arrow_forward
- A 1.00 liter solution contains 0.59 M ammonia and 0.45 M ammonium bromide.If 0.23 moles of perchloric acid are added to this system,indicate whether the following statements are true or false.(Assume that the volume does not change upon the addition of perchloric acid.) A. The number of moles of NH3 will increase. B. The number of moles of NH4+ will remain the same. C. The equilibrium concentration of H3O+ will decrease. D. The pH will remain the same. E. The ratio of [NH3] / [NH4+] will remain the same.arrow_forwardConsider the titration of H2SO4 with NaOH. A 30.0 L sample of H2SO4 requires 0.090L of 0.100 M NaOH. What are the moles ofacid? Number of molecules of the acid? Molarity of Acid? what is the grams of Acid present?A. Moles of Acid?B. Molecules of AcidC. Molarity of AcidD. grams of Acid?arrow_forward4. Calculate the pOH when 35.0 ml of 0.650 M HF is mixed with 15.0 ml of 0.125 M KOH. K, = 7.1 x 10* (Answer must include completed ICE box)arrow_forward
- A 1.00 liter solution contains 0.48 M ammonia and 0.37 M ammonium iodide. If 0.18 moles of hydrobromic acid are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of hydrobromic acid.) A. The number of moles of NH3 will decrease. B. The number of moles of NH4+ will decrease. C. The equilibrium concentration of H3O+ will decrease. D. The pH will remain the same. E. The ratio of [NH3] / [NH4+] will decrease.arrow_forwardCalculate the [H] in a solution that is 0.20 M in NaF and 0.25 M in HF. (Ka -7.2 x 10-4) A. 9.0 X 104 MB. 7.2 x 10-4 MC. 1.2 MD. 0.20 ME. 5.8 ×104 Marrow_forwardA 1.00 liter solution contains 0.58 moles hypochlorous acid and 0.45 moles sodium hypochlorite . If 0.22 moles of nitric acid are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of nitric acid.) VA. The number of moles of HCIO will remain the same. vB. The number of moles of CIO" will decrease. vC. The equilibrium concentration of H30+ will increase. D. The pH will remain the same. vE. The ratio of [HCIO] / [CIO¯] will remain the same.arrow_forward
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