3. (continued) For parts b, c, and d, use the following balanced equation: 2 H3PO4 (aq)...
Write a net ionic equation for the neutralization reaction of H3PO4(aą) with Ba(OH)2(aq). A) 2 H3PO4(aq) + 3 Ba(OH)2(a )--Ba3 (PO4)2(s) + 6 H2O() B) 6H+a)+2 PO43-(aq) +3 Ba2+(ag) + 6 OH-(ag) -+ Ba3(PO4)2)6 H20(1) C) H+(aq) + OH-(aq) → H2O(1) D) 2 H3PO4a)+3 Ba2+a) +6 OH-(a) Ba3(PO42(s)+6H20(0)
The balanced chemical equation presented below is an example of which type of reaction? 2 H3PO4(aq) + 3 Ba(OH)2(aq) Ba3(PO4)2(s) + 6 H2O() a) combination (synthesis) b) double replacement c) single replacement d) decomposition
help me 2. A 20.00 mL sample of H3PO4 (aq) requires 56,01 mL of 0.1885 M NaOH for titration to the third equivalence point. a) What is the molarity of the H3PO. (aq) sample? (4 pts) b) What is the trend in K, values going from H3PO, to H,POto HPO}? What is the reason behind this trend? (2 pts)
Consider the following balanced chemical equation. 2 K3PO4 (aq) + 3 MgBr2(aq) + Mg3(PO4)2(s) + 6 KBr (aq) A 91.06 mL sample of 0.313 M K3PO4 is mixed with 63.81 mL of 1.972 M MgBr2. After reaction, what is the concentration of the excess reactant (in M)?
please show all work neatly 5. (2 pts) Consider the following acids and their dissociation constants HPO4-2(aq) + H2O.. H3O"(aq) + PO4-3(aq) Ka-2.2x 10.13 HCOOH(aq) H20 H3O (a) HCOO (aq) Ka = 1.8x10-4 a. Which is the weaker acid, HPO42 or HCOOH? b. What is the conjugate base of, HPO42 or c. Which acid has the weaker conjugate base? d. Which acid produces more ions? 6. (2 pts) Write a balanced equation for the neutralization of H3PO4(aq) and NaOH(aq) (3...
b. KHCO3 → c. NaOH + H3PO4 → d. Ca + CuCl2 → e. Na2CO3 + AlBry 6. Indicate whether the following ionic compounds are soluble (sol) or insoluble in (insol) in water. Use the Solubility Rules for lonic Compounds on page 154 in your lab manual. (3 pts total) a. (NH4)2S b. Fe(OH)3 c. BaCrO4 7. Convert the following word equations into balanced chemical equations. (2 pts each) a. calcium metal (s) + water (1) calcium hydroxide (aq) +...
1. Consider the following equation: Ca(OH)2(s) + 2HCl(aq) + CaCl2(aq) + 2 H20(1).Solve the following questions based on the above questions, a. What type of chemical reaction is taking place? b. How many liters of 0.100 M HCI would be required to react completely with 5.00 grams of calcium hydroxide? (5 pts) Show the work. c. If I combined 15.0 grams of calcium hydroxide with 75,0 mL of 0.500 M HCI, how many grams of calcium chloride would be formed?...
4 4. a) Parts (a) and (b) below are separate independent problems For each of the following, write a balanced net-ionic equation for the acid-base neutralization reaction that occurs (omitting any spectator ions), and determine the value of the equilibrium constant K for the reaction. Be sure to include phases (such as (aq) or ()) in your reactions. The first one is done for you as an example. (8 pts) Example: Solutions of HBr (ag) and KOH (aq) are mixed...
8 The Following reaction is classified as: 2HCl(aq) + Ba(OH)2(aq) → BaCl(aq) + 2 H20(0) b) precipitation reaction oxidation-reduction reaction d) acid-base neutralization reaction 9. c) single replacement What is the volume of 0.1220 M HNO, solution required to completely neutralize 17.50 ml of 0.1211M NAOH? Reaction is: HNO, (aq) + NaOH(aq) -NaNO, (aq) + H:0 (aq) a) 17.37 ml b) 16.31 ml. c) 15.39 ml. d) 17.84 mL 10. Which one of the following reactions is the reduction reaction?...
1. Consider the following equation: Ca(OH)2(8) + 2HCl(aq) - CaCl(aq) + 2 H2001) Solve the following questions based on the above questions a. What type of chemical reaction is taking place? b. How many liters of 0.100 M HC would be required to react completely with 5.00 grams of calcium hydroxide? (5 pts) Show the work. c. II combined 15.0 grams of calcium hydroxide with 75,0 mL of 0.500 M HCI, how many grams of calcium chloride would be formed?...