Complete and balance the following equations. SrBr2(aq) + _____ Na2S(aq) --> B. A. If no reaction occurs, write No Rxn. (Please give a detailed explanation) ______K2CO3(aq) + Mg(NO3)2(aq) -->
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- 8. The following questions concern the reaction HA(aq) + B(aq) 2 HB1†(aq) + A1-(aq). What can you say about: (a) the magnitude of K for this reaction (K >> 1 or K > solution that results from reacting equal mole quantities of HA with B, when [HB1*] or [HA] << [HB1*]), and (c) the pH of the (a) K (b) Relative concentration (c) pH HA is a weaker acid than HB1+. HA is a weak acid and B is a strong base. HA is a strong acid and B is a strong base. HA is a strong acid and B is a weak base.17. Arrange the compounds in each series in order of increasing acid strength: (a) AsH3, HBr, KH, H₂Se; (b) H2SO4, H2SeO3, H2SO4 Give detailed Solution. don't give Handwritten answer 18. Determine whether aqueous solutions of each of these salts are acidic, basic, or neutral:Balance the equations under acidic solution. (step by step) a. PbO2 + Hg ↔️ Hg22+ + Pb2+ b. Al + Cr2O72- ↔️ Al3+ + Cr3
- Calculate the concentrations of [H3O+], [HSO4-] and [SO42-] in 0.50 M sulfuric acid solution atequilibrium.Complete the charge balance equation for an aqueous solution of H₂CO3 that ionizes to HCO3 and CO3-. [OH] || [H+] C [Co/3-] + Answer Bank [H₂CO3] [HCO3] + ☐ 2 [CO3-] 2[H+] 3[H+]1. What is the pH of a buffer prepared by mixing 100 ml 0.050 mM NaH2PO4 and 25 ml 0.075 mM NɑżHPO4? (pKai=2.2; pKo2= 7.21; pKa3=12.7)
- Calculate the pH of a 0.10M solution of NaHSO4 solution taking into account activity (Ka2 = 1.92 for H2SO4).Complete the charge balance equation for an aqueous solution of H₂CO3 that ionizes to HCO3 and CO2-. [H+] || [OH-] 2[CO3-] + Answer Bank 2[H+] [HCO3] + D 3[H+] [CO] [H₂CO3]A student dissolved a compound in water and added hydrochloric acid. No precipitate formed. Next, she bubbled H2S into this solution, but again, no precipitate formed. However, when she made the solution basic with ammonia and bubbled in H2S , a precipitate formed. Which of the following are possible as the cation in the compound? - CA2+ - Ag+ - Cd2+ - Mn2+
- Complete the balanced dissociation equation for the compound below in aqueous solution. If the compound does not dissociate, write NR after the reaction arrow. HCIO,(aq) – 4- 2- n2+ 3+ D 4+ + 1 3 4 6. 7 8 Os O8 (s) (1) (g) (aq) NR CI Reset • x H,O Delete x H̟O 2 11 3. 2. +a. What cations may be present in a pale blue solution that turns deep blue and forms a white precipitate upon 6M NH3(aq)? b. A white solid dissolves in water to form a neutral solution. No precipitate forms when the solution is treated with a solution of NH4Cl/ NH3 buffer, nor when (NH4)2S is added. When the solution is acidified with HC2H3O2 and K2CrO4 is added a yellow precipitate forms. This precipitate dissolves upon addition of concentrated HCl. Acidification of a solution of the solid with HNO3 followed by addition of AgNO3 causes formation of a white precipitate. What is the identity of the original solid?Calculate the equilibrium constant, Kc, of the reaction: HCO3-(aq) + HCO3-(aq) ↔ H2CO3(aq) + CO32- , Kc = ? Based on your result, do you expect this reaction to occur in the left-to-right direction?