2. Determine a recipe to prepare 200 mL of 20 mM phosphate buffer, pH 6.6, from 0.5 M starting stock solutions. ml of 0.5 M Na2HPO4 (A) ml of 0.5 M NaH2PO4 (HA) Bring to 150 ml with deionized H₂O -110. instructions
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- Please don't provide handwritten solution .....If a 0.3 M solution of NaOH was used to titrate 100 mL of 0.3 M solution of CH3COOH (Ka =1.8 x 10 -5) and the following volumes of NaOH were recorded: 102, 97, 99, 98, 101, 106 mL. The pH Value is………………when added 99.0 mL of 0.3 M NaOH The pH of the solution at the equivalence point more than 7 Because................................... Calculate the 99% confidence limits of the mean? And use them to decide whether there is any evidence of systematic error? [ hints: For N=6 and the 99 % confidence interval, the value of t is 4.03].Hh.87.
- C4Homework: A 1.2gm sample of a mixture of (Na₂CO3+ NaHCO3) is dissolved and titrated with 0.5N HCl. With phenolphthalein, the endpoint is at 15ml while after further addition of methyl orange a second endpoint is at 22ml. Calculate the percentage composition of the mixture. Homework: What mass of Ca(OH)2 is present in a sample if it is titrated to its equivalence point with 44.02 mL of 0.0885 M HNO3? The balanced chemical equation is as follows: 2HNO3 + Ca(OH)2 → Ca(NO3)2 + 2H₂O4. In the titration of15.00 mL of 0.200 M HC with 0.100 M NaOH, calculate the pH after the addition of the following volumes of titrant (mL) ; (a) 0.00; (b) 10.00; (c)14.50 ; (d) 15.00; (e) 15.50: (f) 20.00 mL.
- All boxes pleaseQ:3-3 Consider a 1.00 L buffer made by adding 0.140 mol cyanic acid HCNO, and 0.110 mol potassium cyanate ,KCNO, to sufficient water. Calculate the pH a buffer (a) Before any acid or base is added; (b) after the addition of 0.015 mol of HNO3; (c) After the addition of 0.015 mol of KOH. In parts (b) and (c) assume the volume does not change . pka(HCNO)=3.48; ka(HCNO)= 3.3 X 104.Calculate the pH during the titration with NaOH after addition of: a) 50.00 mL of 0.1000 mol L-1 NaOH to 50.00 mL of 0.1000 mol L-1 CH3COOH (Ka= 1.75 x 10-5). b) Based on the table below, which indicator (A, B or C) is most appropriate to monitor this titration? Explain. Indicator A B C pKIndicator 3.8 9.3 5.0 Actual Transition Range (pH) 3.0 to 4.6 3.0 to 4.6 4.4 to 6.2
- Be sure to answer all parts. Find the pH during the titration of 20.00 mL of 0.1000 M butanoic acid, CH3CH₂CH₂COOH (K₁-1.54 x 10-5), with 0.1000 M NaOH solution after the following additions of titrant. (a) 15.00 mL: pH = (b) 20.60 mL: pH = (c) 26.00 mL: pH = GuiCarbonic acid (H2CO3) is a diprotic acid. For the titration of 50.00 mL of0.0100 M H2CO3 with 0.0100 M NaOH, calculate the pH of the solution (i) before the addition of any NaOH; (ii) at the first endpoint where [H+] ~ (K1K2)1/2; (iii) at the second endpoint; (iv) after the addition of 150.00 mL NaOH.Be sure to answer all parts. Find the pH during the titration of 20.00 mL of 0.1000 M triethylamine, (CH3CH2)3N (K₁ = 5.2 × 10-4), with 0.1000 M HCl solution after the following additions of titrant. (a) 11.00 mL: pH = (b) 20.10 mL: pH= = (c) 29.00 mL: pH = X X X
