A 110.0value - mL buffer solution is 0.255M in NH3 and 0.395 M in NH4Br. The Kb alue for NH3 is 1.76 x 10^-5. What mass of HCI could be handled before the pH falls below 9.00 ?
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- What would be the working stock concentration (in molarity) if you diluted 250 uL of a stock concentration of 10 uM in a total volume of 1 mL?Consider the titration of 50.00 mL of 0.160 M NH3 with 0.200 M HCl. Calculate the pH at the following volumes of the titrant: VT = 0.00 (Initial Stage) VT = 20.00 VT = 30.00 VT = 40.00 (Equivalence Point Stage) VT = 45.00 Kb = 1.76 x 10-5A concentrated lidocaine solution contains lidocaine 1 g/5 mL. How many milliliters of this injection should be used to prepare a 500 mL IV infusion containing 8 mg/mL of lidocaine in D5W? Do not round.
- Titration of a 12.0 mL solution of HCl requires 22.4 mL of 0.12 M NaOH. What is the molarity of the HCl solution?50X TBE is 87 mM Tris-borate and 4 mM EDTA at pH 8.3. What is the molarity of each of the chemicals in 1X TBE buffer?If 4 mL of 1 M NaOH is added to 100 mL buffer, would it still be a usable buffer according to the conventions? Explain why or why not.
- What is the pH of the buffer 0.17 M Na2HPO4/0.25 M KH2PO4?As a technician in a large pharmaceutical research firm, you need to produce 200. mL of 1.00 M potassium phosphate buffer solution of pH = 6.96. The pKa of H2 PO4 is 7.21. %3D You have the following supplies: 2.00 L of 1.00 M KH2PO4 stock solution, 1.50 L of 1.00 M K2HPO4 stock solution, and a carboy of pure distilled H2O. How much 1.00 M KH2PO4 will you need to make this solution? Express your answer to three significant digits with the appropriate units. > View Available Hint(s) HẢ Volume of KH2PO4 needed = Valıxe Units SubmitIf 400 mL of a 20% w/v solution were diluted to 2 L, what would be the finalpercentage strength?
- You record the absorbance of your unknown BSA sample at 0.276. What is the concentration in ug/mL of the unknown assuming you have a standard curve with the line of best fit with y=0.0001x+0.0038 as its equationAn aqueous solution contains 0.34 M potassium cyanide. One liter of this solution could be converted into a buffer by the addition of: (Assume that the volume remains constant as each substance is added.) 0.34 mol HCI04 0.16 mol NaOH 0.33 mol KCIO4 0.16 mol HCIO4 0.33 mol HCNA buffer contains 0.015 mol of lactic acid (pK₁ = 3.86) and 0.080 mol of sodium lactate per liter. H₂C OH Lactic acid OH Calculate the pH of the buffer. H₂C. Calculate the change in pH after adding 9.0 mL of 0.10 M HCl to 1.0 L of the buffer. O OH Sodium lactate Calculate the change in pH after adding 9.0 mL of 0.10 M HCl to 1.0 L of pure water. O Na+ buffer pH: buffer pH change: water pH change: units units