7) It is the value of a2 for a solution with pH =4.40 containing 0.150 M malonic acid (HOOCCH;COOH, Kal=1.41 x 10, Ka2=2.00 x 10 ): a.0.0350 b. 0.0466 c. 0.0262 d. 0.0670 e. 0.927
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- 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.Calculate the volume, in milliliters, of 0.170 M NaOH that must be added to 319 mL 0.0439 M 3‑(?N‑Morpholino) propanesulfonic acid (MOPS) to give the solution a pH of 7.55. The pKa of MOPS is 7.18. NaOH volume = mLa) 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.
- HIn(aq) + H2O(l) H3O+(aq) + In-(aq)red yellowThe acid base indicator methyl orange is red at pH values below 3 and is yellow at pH values above 6. Usingyour knowledge of pH, indicators and pKa values, predict the pKa of methyl orange.What would the pH be after addition of 10.09 mL of 0.1000 M HCl to 25.00 mL of 0.1000 B (a weak base, Kb = 3.26e-6)?a) At temperature 25°C, 0.02 M hydrazine, N2H4 solution is 0.69% ionised. Calculate the i. Concentration of OH- ion ii. ionisation constant, Kb b) Calculate the mass of sodium benzoate, C6H5COONa that should be added to 500 mL of 0.2M aqueous benzoic acid, C6H5COOH solution to produce a buffer with pH 3.50?[ Ka for C6H5COOH = 6.3 x10-5] c) When a 1 x 10-3 moldm-3 solution of CaCl2 is mixed with an equal volume of a 1 x 10-3 moldm-3 solution of Na2SO4, will precipitate form? (Ksp CaSO4= 2 x 10-5) Do you mean that pH? That was all the given information the question gave.. I don't understand how to use the ionised part the most
- please help me answer a nad then b a. In the laboratory, a general chemistry student measured the pH of a 0.590 M aqueous solution of ethylamine, C2H5NH2 to be 12.185. Use the information she obtained to determine the Kb for this base. Kb(experiment) =______ b. Now, Write the Ka expression for an aqueous solution of nitrous acid: (Note that either the numerator or denominator may contain more than one chemical species. Enter the complete numerator in the top box and the complete denominator in the bottom box. Remember to write the hydronium ion out as , and not as ) Ka =Consider that benzoic acid is a weak acid which has a Ka of 6.3 x 10-5 . C6H5COOH → C6H5COO- + H+ Calculate the [H+ ] ion concentration of a 0.04 M benzoic acid solution. Use your findings from above, determine the pH of the solution.Calculate the pH at which pilocarpine (basic drug) starts toprecipitate from a 2% w/v aqueous solution of itshydrochloride salt.Given the following data:The solubility of pilocarpine in water=0.207 % w/vThe pka of pilocarpine =6.61The molecular weight of pilocarpine=208.3 g/lThe molecular weight of pilocarpine hydrochloride = 244.8 g/l
- A particular solution is 0.05M with respect to ethanoic acid and 0.2M with respect to sodium ethanoate (Ka for ethanoic acid = 2 x 10-5moldm-3). What is this type of solution called? Calculate the pH of the solutionA physician wishes to prepare a buffer solution at pH = 3.82 that efficiently resists changes in pH yet contains only small concentrations of the buffering agents. Determine which one of the following weak acids, together with its sodium salt, would probably be best to use: m-chlorobenzoic acid, Ka= 1.04 × 10-4 ; p-chlorocinnamic acid, Ka=3.89 × 10-5 ; 2,5-dihydroxybenzoic acid, Ka = 1.08 ×10-3 ; or acetoacetic acid, Ka= 2.62 × 10-4 . Explain.Calculate the volume, in milliliters, 0.170 M NaOH that must be added to 303 mL 0.0471 M 3‑(?N‑Morpholino) propanesulfonic acid (MOPS) to give the solution a pH of7.55. The pKa of MOPS is 7.18.