A beaker contains 100. mL of the buffer solution. What is the resulting pH when 50.0 mL of 0.4 M HNO3 is added to the buffer? H₂PO; HPO2- 0.50 M; 0.50 M Кан,род pH after strong acid added = [?] = 6.23 x 10-8 pH of Soln w/ Acid Enter
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- 10. 50 cm3 of 0.05 M weak acid solution is titrated with 0.1 M NaOH solution. The measured pH valuesare 7.345 and 7.497 at the consumptions of 6.0 and 6.1 cm3, respectively. What value of the buffer capacity can be calculated in the solution at pH = 7.421?11. Based on the data given in question 10, what is the total concentration of the anion of the weak acid atthe given point?(a) I f t he molar solubilit y o f CaF2 at 35 °C i s1.24 x 10-3 mol/L, what is Ksp at this temperature? (b) It isfound that 1.1 x 10-2 g SrF2 dissolves per 100 mL of aqueoussolution at 25 °C. Calculate the solubility product forSrF2. (c) The Ksp of Ba(IO3)2 at 25 °C is 6.0 x 10-10. What isthe molar solubility of Ba(IO3)2?What is the solubility of silver iodide in grams per milliliter at a temperature at which the Ksp of AgI is 1.52×10-16?
- A 25.0-mL aliquot of vinegar was diluted to 250 mL in a volumetric flask. Titration of 50.0-mL aliquotsof the diluted solution required an average of 35.23 mL of 0.08960 M NaOH. Express the acidity of the vinegar in terms of the percentage (w/v) of acetic acid.Calculate the pH at the stoich iometric po int of the titration of 25.00 cm3 of 0.150 M lactic acid with 0.188 M NaOH(aq) .Given the titration reaction: Tl3+ + 2Fe2+ « Tl+ + 2Fe3+. Tl3+ + 2e- ↔ Tl+ E0 = 1.25 V Fe3+ + e- ↔ Fe2+ E0 = 0.771 VWhat is potential of 25.00 mL of 0.100 M Tl3+ after adding the following volumes of 0.100 M Fe2+:a. 10mLb. Equivalence pointc. 65mL
- 100 ml 0.10M AgNo3 is added 100 ml of 0.12 M Nacl (ksp agcl = 1x10^-10) 1. CALCULATE THE NUMBER OF MILLIGRAMS of Ag+ not precipitate (m. W of ag = 107.8 g/mol) 2. If precipitate of agcl is washed with 200 ml of water at 25 c what is yhe maximum number of milligrams of agcl that could be lost by solubility in the wadh water? ( m. W agcl = 143,32 g /mol)You are titrating 1.0 mL of a saturated calcium iodate Ca(IO3)2 solution in 0.0100 M potassium iodate KIO3 solution. At the endpoint, 0.78 mL of titrant (0.200 M Na2S2O3) was added. What is the total concentration of IO3-?A 25.0-mL aliquot of vinegar was diluted to 250 mL in a volumetric flask. Titration of 50.0-mL aliquots of the diluted solution required an average of 25.23 mL of 0.09041 M NaOH. Express the acidity of the vinegar in terms of the percentage (w/v) of acetic acid.
- A buffer solution is created containing 3.25 M acetic acid and 0.550 M sodium acetate. The Ka of acetic acid is 1.77 x 10-5. What is the pH of the solution?A 50.00 mL 0.750 M KOH(aq) is added to a 100.0 mL 0.500 M CH3COOH/NaCH3COO buffer. What is the expected pH of the solution?Calculate the molar solubility of Ag2CrO4 (Ksp = 1.12×10-12) in (a) Pure water: (b) In a 1350 mL solution containing 0.750 M K2CrO4: