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- The formula for tartaric acid is preferably written as H2C4H4O6 rather than as C4H6O6. Explain why.OH- + CH3COOH ==== CH3COO- + H2O. Which of the reactants is an acid?Be sure to answer all parts. What H3O+ concentration corresponds to each pH value: (a) pH = 12; [H3O+] = ×10M (b) pH = 7; [H3O+] = ×10M (c) pH = 9; [H3O+] = ×10M
- 2. HPO42taq) + H2Ou) = H2PO4°(aq) + OH 3. CH3COOH(aq) + H2O) = CH3COOH2*(aq) + OH(aq)Type your answers in all of the blan When sulfurous acid, H,SOgis dissolved in water it.undergoes stepwise dissociation, initially giving up its first proton the in the reaction: H2SO3(aq) + H20(aq) = H30*(aq) + HSO, (aq) The resulting HSO, (aq) species is amphoteric in solution and can thus react with water as either an acid or as a base. The equilibrium expressions below show these 2 scenarios. Identify whether HSO, (ag) behaves as an acid or as a base in these reactions. HSO, (aq) + H20(1) H2SO3(aq) + OH (aq) In this reaction HSO, acts as alan HSO, (aq) + H,0(1) So, (aq) + H30 (aq) in this reaction HSO, acts as a an pe younenwerhare Fullscreen 9:28 PM a S2/2021 prt sc delete home 144 & 7. num lock backspace 6. 8. 7. 8. R pg up home enter F H. K pause ↑ shift end alt ctrl ins 4.9. In the acid-base reaction: F-(aq) + HNO3 (aq) HF (aq) + NO3- (aq), which species is the base?
- Q4. Identify the acids and bases in the following equations and explain your reasoning: a) HCl(R) + NH3(R) → NH,Cl(s) b) HCO3 (aq) + ỞH (aq) → H2O() + CO3²(aq) 5T LígN(aq) + 2NH3(aq) → 3Li*(aq) + 3NH2.(aq) c) d) 2(CH3)2NH(aq) + H2SO4(aq) → 2(CH3)2NH2*(aq) + SO,²"(aq) e) CH3CH2OH(aq) + KOH(aq) → CH3CH2OK(aq) + H2O(1) f) PH4Cl(aq) + HCOONA(aq) → PH3(aq) + NaCl(aq) + HCOOH(aq) स्मजील 8) NH2CH2COOH(aq) + NH½CH(CH2SH)COOH(aq) → NHCH2COO'(aq) + *NH3CH(CH2SH)COO(aq)The compound HA is an acid that is soluble in water. Which of the "beakers" below shows HA behaving as a weak acid in water?Phthalic acid (H,C3H,O4, abbreviated H,Ph) is a diprotic acid. Its ionization in water at 25°C_takes place in two steps: H¿Ph(aq) + H20(e)=H;0* (aq) + HPH¯(aq) Ka1 = 1.26 × 10~³ %3D HPH¯(aq) + H,O(e)2H;0*(aq) + Ph² (aq) K22 3.10 × 10¬6
- (Q6) If the equilibrium pH of an aqueous solution is 1.72 and the solution is 0.433 M in formic acid, what is the percent ionization?(a) pH is defined as the negative logarithm of hydrogen ions (H+), mathematically it can be expressed as pH= log(1/H+); (b) a solution containing 1x10-1 H+ mol/L has lower H+ concentration compared to a solution containing 1x10-5 H+ mol/L. * A if a is correct B if b is correct C if both statements are correct D if neither statement a nor b are true(Q7) If the initial concentration of the weak base ammonia in a solution is 0.401 M and the solution is 1.39 % ionized, what is the solution pH?
