a ) HI ( aq ) + NH3 ( aq). ---->. NH4I (s)
B.) NaOH ( aq ) + NaHSO4 ( aq ). ---- >. Na2SO4 ( aq ) + H2O ( l)
C.)LiNH2 (aq) + CH3CO2H (aq). ----> CH3CO2- LiNH3 +.
Final product = CH3CO2LiNH3 (. Weak acid + weak base )
D. )Na2CO3 (aq) + 2 KCN(aq). ---->. K2CO3 (s) + 2 NaCN (aq)
1) Write the equation that would occur when each of the following pairs of chemicals are...
A) Which of the following pairs cannot be mixed together to form a buffer solution? Why? A. NH3, NH4Cl B. KOH, HF C. NaC2H3O2, HCl D. H3PO4, KH2PO4 E. RbOH, HCl I already know the answer is E. I want help understanding when we can rule out choices B and C. B) For a solution equimolar in HCN and NaCN, which statement is false? Without giving all the choices, the false choice is "The [H+] is larger than it would...
Please write out equation used and indicate the values used where in each equation. ICE tables, where applicable. 2) Calculate the pH of each of the following solutions. (5 pts each) a) 0.35 M H2SO4 b) 0.35 M HCN c) 0.35 M KOH d) 0.35 M CaBr2 e) 0.35 M KCN f) 0.35 M CH3CH2NH2 g) 0.35 M NaHSO4 h) 0.35 M CH3CH2NH3Br
How would you calculate the pH of solutions 1-4? Calculate the theoretical value of the each solution mixture (A, B, C, D) using ICE table or Henderson Hasselbalch equation and compare your numbers with the lab numbers Data Table Test tube Beaker А pH 3.5 Chemicals mixture 1M 25 ml CH3CO2H in water 1M 25 ml NH4OH (NH3 in water) 1M 25 ml CH3CO2H+ 2 g CH3CO2Na 1M 25 ml NH4OH + 2 g NH4Cl Universal indicator color light green...
Write the balanced net ionic equation for the reactions that occur when the given aqueous solutions are mixed. Include the physical states. A. silver nitrate, AgNO3, and magnesium bromide, MgBr, net ionic equation: B. perchloric acid, HCIO , and potassium hydroxide, KOH net ionic equation: C. ammonium sulfide, (NH),S, and cobalt(II) chloride, COCI, net ionic equation:
Write the balanced net ionic equation for the reactions that occur when the given aqueous solutions are mixed. Include the physical states. A. silver nitrate, AgNO3 , and magnesium bromide, MgBr2 net ionic equation: B. perchloric acid, HClO4 , and potassium hydroxide, KOH net ionic equation: C. ammonium sulfide, (NH4)2S , and cobalt(II) chloride, CoCl2 net ionic equation:
Write the balanced net ionic equation for the reactions that occur when the given aqueous solutions are mixed. Include the physical states. A. silver nitrate, AgNO, and magnesium bromide, MgBr net ionic equation: B. perchloric acid, HCIO, and potassium hydroxide, KOH net ionic equation: C. ammonium sulfide, (NH),S, and cobalt(II) chloride, CoCl, net ionic equation:
67. Write the balanced formula equation for the acid-base reactions that occur when the following are mixed. a. potassium hydroxide (aqueous) and nitric acid b. barium hydroxide (aqueous) and hydrochloric acid
Write the complete and net ionic equations for the reactions that would occur if the following pairs of solutions were mixed. Be sure to indicate whether reaction products are solid or dissolved in water. 2. (1) BaCl2(aq) +KIO3(aq)→ (2) Sr(NO3)2(aq) + Na2SO4(aq) → (3) Pb(NO3)2(aq) + NaOH(aq)→ (4) CuSO4(aq) + Na2C2O4(aq) →
(c) A slightly ionized compound, usually water 2. Write the equation for the decomposition of sulfurous acid. H₂SO₄ (aa) H2O(l) + 5O2 (9) 3. Using three criteria for double displacement reactions, together with the Se Table in Appendix 5, predict whether a double displacement reaction will occur example below. If reaction will occur, complete and balance the equation, prope cating gases and precipitates. If you believe no reaction will occur, write "no read the right-hand side of the equation. All...
Write the balanced equations (all three types) for the reactions that occur when the following aqueous solutions are mixed. (Use the lowest possible coefficients. Include states-of-matter under the given conditions in your answer.) molecular equation: complete ionic equation: net ionic equation: (a)perchloric acid [HClO4(aq)] and iron(III) hydroxide. (b) ammonia (aqueous) and hydroiodic acid. (c) calcium hydroxide (aqueous) and hydrochloric acid. (d) solid silver hydroxide and hydrochloric acid