Solid CO2 (0.40 mol) is reacted with CH3MgBr (0.29 mol) in ether solvent. The product of the reaction is isolated in aqueous solution (assume 100% yield) and excess CO2 is removed. Subsequently, HCI (aq) (0.13 mol) is added. What is the pH of the solution that results? Notes: You will need to look up a pk for this question and report your answer to 2 decimal places.

Carbonate (H2CO3/HCO3-) buffers are important in regulating the pH of blood at 7.40.  Note that the Ka for H2CO3 is 4.3 x 10-7. When a person exercises, muscle contractions produce lactic acid.  Moderate increases in lactic acid can be handled by the blood buffers without decreasing the pH of blood.  However, excessive amounts of lactic acid can overload the blood buffer system, resulting in a condition called acidosis if the blood pH falls to 7.35 or lower. Suppose a patient’s normal blood sample contains [H2CO3] = 0.0015 M and [HCO3-] = 0.0129 M.  If this patient exercises enough to produce 0.0010 mole of H3O+ per 1 L of blood due to production of lactic acid, would they be diagnosed with acidosis?

2. DETAILS PREVIOUS ANSWERS NCSUGENCHEM202LABV1 7.POST.02. Given that carbonic acid, H₂CO3, has a pka1 = 6.37 and a pka2 = 10.33, answer the following. (a) If you wanted to make a pH 7 buffer solution starting with NaHCO3(aq), would you add 0.10 M HCl or 0.10 M NaOH? O 0.10 M HCI 0.10 M NaOH (b) If you began with 7.0 mL of 0.17 M NaHCO3, how many mL of your choice from (a) would you need to add to get a pH 7 buffer? 3.94 XML

3. Copy the five sets of data (volume NaOH and pH) from titration #3 into the table on the next page. Calculate the pKa for the unknown weak acid using one set of the data. Show the equations used to calculate concentrations of [A] eq and [HA] eq and show how these values are substituted into the rearranged Henderson-Hasselbalch equation (Eqn. 16.10).

3. A 1.0 M solution of a compound with 2 ionizable groups, i.e. carbonic acid (H₂CO3), has a pH of 6.8. The pka's of the ionizable groups are 6.37 and 10.26. A) Draw the full reaction for titration from the fully protonated to the fully deprotonated form for this compound, place the pka's at the appropriate arrows. B) Draw a titration curve for this compound B) If a biochemist has 100 mL of this solution, and adds 10 mL of 1.0 M NaOH to it, what is the new pH? (Show your work)

[References] Calculate the pH of buffers that contain the acid and conjugate base concentrations listed below. a. [CH3 COOH] = 0.85 M, [CH3 COO¯] = 0.45 M (the pK, for acetic acid is 4.74) pH = b. [H2PO4-] = 0.50 M, HPO,? = 0.20 M (the pK, for H2PO4 is 7.21) %3D pH = c. [HSO;¯] = 1.85 M, SO32| = 0.60 M (the pK, for HSO; is 7.00) с. pH = Submit Answer Try Another Version 5 item attempts remaining

Incorrect Your answer is incorrect. • KC: Your answer is incorrect. • Cacl, Vour answer is incorrect. For each of the following compounds, decide whether the compound's solubility in aqueous solution changes with pH. If the solubility does change, pick the pH at which you'd expect the highest solubility. You'll ind K, data in the ALEKS Data tab. Does enlubility change with pH? hiyhest solubility compound pll 5 pll 6 pll 8 yes O no yes Ba(OH), O no O yes Caci, e no

An initial 0.010 M solution of a weak acid (HA) is measured to have 0.0015 M of its conjugate weak base (A") in solution at CC equilibrium. Calculate the pK, for the weak acid. 2.82 O3.58 O3.65 0.18 0.82

4. Compounds might have more than pKa.  5. We usually prefer to prepare buffers from alkaline origin compounds.  6. The pH of a buffer solution containing .1 M acetic acid and 0.1 M sodium acetate? (Ka for acetic acid = 1.75 ×10-5) is 3.9.  7. The pH of a solution containing ephedrine 0.1 M and ephedrine HCI 0.01 M? (Kb for ephedrine = 2.3 x 10-5) is 7.99.  8. The maximum buffer capacity for solutions can be achieved when the required pH double than pKa of the acid..  9. When one of the buffer components is depleted completely the solution lose its buffering capacity and can no longer resist the change in pH.  10. At a hydrogen ion concentration of 1.75 x 10-5, what is the capacity of a buffer containing 0.10 mole each of acetic acid and sodium acetate per liter of solution? (Ka = 1.75 x 10-5 ) is 9.11.

İBRAHİM YAM. O Aia (Alt- G) Yeni. - Gözden Gegir Gorunam Yardım Başvurular Posta Gönderleri 1)) Calculate pKa' according to given equati ons. Dissociation of carbonic acid to bicarbonate ion and a proton: [H] [HCO:] Ka- [Co] [H0] The first equation for the equilibrium between dissol ved CO and water and H;CO3: CO2e +H2O( PH CO; Keg= 3x10-3= H»CO:]| [COo} [HO] The second is for the dissociation of I1- CO: IICO:+H Ka = 1.7x10 - [I1] [HCO;1 H2CO; [H;CO:] H HCO. Co. HCO CO HO HCO The yield equation is: CO. HO DOdak aton 9°C Bu 8 K alt gr