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(6) 0.8203 g NaAc (FW=82.03 g/mol) was fully dissolved into 100.00 mL of 0.050 M HAc solution. Calculate th pH of the soolution.
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- A hypothetical weak acid, HA, was combined with NaOH in the followingproportions: 0,20 mol HA, 0,08 mol NaOH. The mixture was diluted to a totalvolume of 1,0 L and the pH was found to be 4,80. a). What is the pKa of the acid?What happens when too much NaSCN is prepared in solution of mixtures of standard solutions of Fe(NO3)3 and NaSCN, so that [SCN^-] is higher than expected? What does this do to the measured Keq?A weak acid is added to a strong base. The base is neutralized last, giving a mole ratio to acid remaining of 2:3. If Ka is 1.0 x 10-5, what is the ph of the solution?
- ) A truck driver carrying a load of lead nitrate (Pb(NO3)2) lost control of his semi- truck after hitting a patch of ice and crashed the truck into Blue Lake, which was right next to the highway. Despite the best efforts of the emergency workers, several of the crates containing lead nitrate were damaged, and the highly soluble compound dissolved immediately. Assuming the lake is initially at circumneutral pH (7), and that the spill resulted the in a total lead concentration of 10-3 M within the lake. Based on the following information, will PbO(s) precipitate out of Blue Lake. Assume all lead nitrate dissociates into Pb+2 and NO3-, no other sources of lead exist in the lake and that no other reactions besides the equations shown below occur. PbO(s) + 2H+ ⇌ PbO(s) + H+ ⇌ PbO(s) + H2O ⇌ PbO(s) + 2H2O ⇌ Pb2+ + H2O PbOH+ + H2O Pb(OH)2o Pb(OH)3- + H+ logKs0/ksp =14 logK1=3.4 logK2=-0.5 logK3=-12A buffer was made using 0.10 moles of A- and 0.01 moles of HA. If the pKa is 5.71, what is the pH of thebuffer?What will be the pH of a solution when 200ml of 0.1M HEPES in the basic form and 100mL of 0.1 M HEPES in the acid form are mixed together? The pKa of HEPES is 7.55
- 10. 50 cm3 of 0.05 M weak acid solution is titrated with 0.1 M NaOH solution. The measured pH valuesare 7.345 and 7.497 at the consumptions of 6.0 and 6.1 cm3, respectively. What value of the buffer capacity can be calculated in the solution at pH = 7.421?11. Based on the data given in question 10, what is the total concentration of the anion of the weak acid atthe given point?You prepare 250.0 mL of a buffer solution containing 0.550mol of acid and 0.450mol of its conjugate base. If the literature pKa of the acid used is 6.49, what is the expected pH of the resulting buffer solution?A 25.0-mL aliquot of vinegar was diluted to 250 mL in a volumetric flask. Titration of 50.0-mL aliquotsof the diluted solution required an average of 35.23 mL of 0.08960 M NaOH. Express the acidity of the vinegar in terms of the percentage (w/v) of acetic acid.
- 6. If 25.1 mL of 0.109M acid with a pKa of 5.27 is titrated with 0.108 M NaOH solution, what is the pH of the titration mixture after12.0 mL of base solution is added?A 250 cm3 volumetric flask contains exactly 200,0 cm3 of a 0,025 mol.dm3sulphuric acid solution. Thereafter ten (10) sodium hydroxide pellets, eachof mass 0,1 g are dropped into the flask. After the pellets have dissolvedcompletely, the flask is topped to the 250 cm3 mark with water and thecontents are thoroughly homogenised. Determine the pH of the resultingsolution.When adding 25 ml of a pulverizer containing a solution of M (NaOH 0.2) to a beaker containing 50 ml of CH3COOH (0.1M) acid having a value of = 4.76 pka, the acidic function of the resulting solution is equal to?