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Calculate the pH of 50mls of 0.1100M arginine to which 20 mls PH of 0.1005M Hcl have been added.
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- In the determination of the water hardness of a river water sample, the pH of the sample was adjusted to 12 instead of 10. Is there a positive error, negative error, no effect, or error could not be determined In terms of the ppm CaCO3 of sample?calculate the pH of 50.0 mLs of 0.10 M arginine hydrochloride to which 50.0 mLs of 0.10 M NaOH have been added.Find the pH of a solution 2.0 M in ethylamine CH3CH2NH2. For CH3CH2NH2 Kb=5.6x10-4. Explain step by step as you set up the equation and what each element represents.
- The measured pH of a 0.100 M solution of triethylamine (NEt3) is 11.68. What pKa of triethylammonium (HNEt3+) is implied by this data? Enter your response to the nearest 0.01.A 25.0cm3 sample of a 0.1 mol/dm3 solution of ethanoic acid (ka = 1.8 x 105) was titrated with 0.1 mol/dm3 sodium hydroxide. Calculate the pH of ethanoic acid.a) Why can you not prepare a solution of pH = 8 by diluting sufficiently a 0.01 M solution of HCl with water? b) You could determine Ka for benzoic acid by measuring the pH of a 0.010 M solution of benzoic acid. Why is the graphical method used in this experiment a better way of determining Ka? c) List the measurements along with their uncertainties made in the determination of the molar mass of benzoic acid. Calculate the uncertainty in the mola r mass of benzoic acid determined by the titration.
- a solution was prepared by dissolving 25.0 grams of ethanoic acid CH3COOH with 15 grams of sodium ethanoate CH3COONa in a volume of 750 ml. The dissociation constant of ethanoic acid is 1.8 × 10-⁵. Find the pH of the solution30ml of 0.06M solution of protonated form of anion amino acid methionine (H2A+) is treated with0.09M NaOH.calculate pH after addition of 20 ml of base.pKa1=2.28 and pKa=9.2 please answer this question .with explanationDerive the titration curve when titrating 100.0mL of 0.100M weak base aniline (pka = 4.601) with 1.000M HClO4 using the following volumes of acid, 0.00mL, 2.00mL, 5.00mL, 8.00mL, 10.00mL, 13.00mL? (find the pH values and make a graph of pH vs VHClO4
- Ethylamine (C2H5NH2) has a Kb value of 4.5x10–4. Calculate the pH of a buffer solution that is 0.00789 M ethylamine and 0.00546 M ethylammonium chloride.Calculate the volume, in milliliters, of 0.170 M NaOH that must be added to 247 mL 0.0581 M 3‑(N‑Morpholino) propanesulfonic acid (MOPS) to give the solution a pH of 7.55. The pKa of MOPS is 7.18.1Upon the addition of 30.00 mL of 0.350 M HCl to a 80.00-mL of the weak base amine (Kb = 4.95 x 10-10) whose concentration is 0.530M, the resulting pH is then equal to 8.80. True or False? 2.When 100 mL of a 1.0M strong acid is 50% titrated with 1.0M strong base, the volume of the base should be added is 50mL and this corresponds the equivalence point. True or False? 3. The pH of a buffer can be calculated using the formula: 14-pOH = pKb + log of [proton acceptor]/[acid component]. True or False?