Q) Calculate the pH of benzoic acid solution (25 mL, 0.1 M) after the addition of the following volumes of KOH (0.1 M). [ka of benzoic acid = 6.5 x10 1 a) 0 mL b) 10 mL c) 25 mL d) 40 mL Submiesion status
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- 1) Calculate the required gram of Tris-Hcl to prepare 1M, 100 ml Tris-HCl (Tris Stock) with mol and Molarity formula. 2)Calculate the required gram of EDTA to prepare O.5M, 100 ml EDTA (EDTA stock) mol and Molarity formula. 3.) Calculate the required volume of Tris Stock to prepare buffer A which contains 25 mM Tris-Hcl with final volume is 100 ml by using M1V1 =M2V2 formula 4) Calculate the required volume of EDTA stock to prepare buffer A which contains 10 mM EDTA with final volume is 100 ml by using M1V1 =M2V2 formula 5)Do the same for Buffer B calculationsA 35 mL of solution of hydrochloric acid is neutralized by 15 mL of 0.5 M potassium hydroxide. What is the concentration of hydrochloric acid? The balanced equation is HCI + KOH - H,O + KCI O 0.75 M O 0.25 M O 0.214 M O 0.786 MDescribe the preparation of 2.00 L of 0.100 M glycine buffer, pH 9.0, from glycine and 1.00 M NAOH. What mass of glycine is required, and what volume of 1.00 NaOH is required? The appropriate pK, of glycine is 9.6.
- Describe the preparation of 2.00 L of 0.100 M glycine buffer, pH 9.0, from glycine and 1.00 M NaOH. What mass of glycine is required, and what volume of 1.00 NaOH is required? The appropriate pKa of glycine is 9.6Consider 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 10-5If a pharmacist needs to prepare a bacterial suspension with a concentration of 2.4x10^2 cfu using 1 mL of 2.4 x 10^4 bacterial suspension, what size of volumetric flask will she/he be needing?
- What is the pH of a 0.25 M solution of acetic acid, Ka = 1.8 x 105. What percentage of the acid is dissociated?Calculate the pH of the resulting solution if 23.0 mL of 0.230 M HCl(aq) is added to 33.0 mL of 0.230 M NaOH(aq). pH = Calculate the pH of the resulting solution if 23.0 mL of 0.230 M HCl(aq) is added to 13.0 mL of 0.330 M NaOH(aq). pH=2. 500 ml of a 0.1 M sodium phosphate buffer with pKa = 7.21, is diluted %3D a) How would you dilute this buffer 100 times to make a final volume of 50 ml? Show the ratios to be added together. b) Calculate the pH of the buffer when it is diluted with dH20 c) Calculate the pH of the buffer when it is diluted with 0.3 M KCI %3D 3. What is the normality of a 5 M phosphoric acid (SG = 1.88 g/cm³; 85% solution has a Mr of 98 g/mole
- 40.00 mL of 0.1100 M HCl is diluted to 100 mL with H2O and titrated with 0.1M NaOH. Calculate the pH after addition of the following volumes(mL) of titrant. d) 40.00 e) 43.95 f) 44.00 g) 44.05 h) 50.00. Plot the titration curve. Select an indicator from the table found in your book.A 5% dextrose in 1/2 normal saline (D5 1/2 NS) solution is commonly administered to patients needing post-operative IV fluids. How could you prepare 500 mL of this solution? Dextrose is 5% (m/v) and the NaCl is 0.45% (m/v).how many grams of sr(no2)2 are needed to make 200 ml of 0.300M solution of sr(no2)2