Problem

Great Lakes Chemical Company produces bromine, $\…

01:19

Problem 28 Medium Difficulty

Write the molecular, total ionic, and net ionic equations for the following reactions:
(a) $\mathrm{Ca}(\mathrm{OH})_{2}(a q)+\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q) \longrightarrow$
(b) $\mathrm{H}_{3} \mathrm{PO}_{4}(a q)+\mathrm{CaCl}_{2}(a q) \longrightarrow$

Answer

(a)
Molecular
Ca(OH) $_{2}(a q)+2 \mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q) \longrightarrow \mathrm{Ca}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{2}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l)$
Complete lonic
$\mathrm{Ca}^{2+}(a q)+2 \mathrm{OH}^{-}(a q)+2 \mathrm{H}^{+}(a q)+2 \mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}^{-}(a q) \longrightarrow \mathrm{Ca}^{2+}(a q)+\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}^{-}(a q)+$
Net lonic
$\mathrm{H}^{+}(a q)+\mathrm{OH}^{-}(a q) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l)$
(b)
Molecular
$2 \mathrm{H}_{3} \mathrm{PO}_{4}(a q)+3 \mathrm{CaCl}_{2}(a q) \rightarrow \mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}(s)+6 \mathrm{HCl}$
Complete Jonic
$6 \mathrm{H}^{+}(a q)+2 \mathrm{PO}_{4}^{3-}(a q)+3 \mathrm{Ca}^{2+}(a q)+6 \mathrm{Cl}^{-}(a q) \longrightarrow \mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}(s)+6 \mathrm{H}^{+}(a q)+\mathrm{Cl}$
Net Ionic
$2 \mathrm{PO}_{4}^{3-}(a q)+3 \mathrm{Ca}^{2+}(a q) \longrightarrow \mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}(s)$

Top Chemistry 101 Educators

Allea C.

University of Maryland - University College

Watch More Solved Questions in Chapter 4

Problem 1

Problem 2

Problem 3

Problem 4

Problem 5

Problem 6

Problem 7

Problem 8

Problem 9

Problem 10

Problem 11

Problem 12

Problem 13

Problem 14

Problem 15

Problem 16

Problem 17

Problem 18

Problem 19

Problem 20

Problem 21

Problem 22

Problem 23

Problem 24

Problem 25

Problem 26

Problem 27

Problem 28

Problem 29

Problem 30

Problem 31

Problem 32

Problem 33

Problem 34

Problem 35

Problem 36

Problem 37

Problem 38

Problem 39

Problem 40

Problem 41

Problem 42

Problem 43

Problem 44

Problem 45

Problem 46

Problem 47

Problem 48

Problem 49

Problem 50

Problem 51

Problem 52

Problem 53

Problem 54

Problem 55

Problem 56

Problem 57

Problem 58

Problem 59

Problem 60

Problem 61

Problem 62

Problem 63

Problem 64

Problem 65

Problem 66

Problem 67

Problem 68

Problem 69

Problem 70

Problem 71

Problem 72

Problem 73

Problem 74

Problem 75

Problem 76

Problem 77

Problem 78

Problem 79

Problem 80

Problem 81

Problem 82

Problem 83

Problem 84

Problem 85

Problem 86

Problem 87

Problem 88

Problem 89

Problem 90

Problem 91

Problem 92

Problem 93

Problem 94

Problem 95

Video Transcript

for this next question, we were asked to write the molecular ionic or complete ionic or total ionic and then the net ionic equations for these two chemical reactions that are provided for the first one, it's calcium hydroxide reacting with acidic acid because we have an acid acetic acid reacting with the hydroxide containing species. The products will be a salt which will be calcium combining with the acetate of acetic acid and water coming from hydrogen reacting with the hydroxide. Once we've identified the products, we then need to identify what the coefficients are. To balance the chemical reaction. We have to assume tapes here, we have one acetate in this one acetic acid. So we're going to need to put a two there. That then gives us two hydrogen is that can combine with the two hydroxide is to produce two waters. Now it's balanced this would be the complete molecular equation. Now that we have a complete molecular equation, we can separate the ionic compounds that are soluble in water into ions. To obtain the total ionic equation one calcium will produce one calcium ion. Two hydroxide will produce two hydroxide and ions. However, the acetic acid, although a weak electrolyte, meaning it is an electrolyte and some of it will separate into ions, well not completely separate into ions. So most of it stays together as molecular acetic acid. So the best representation of acetic acid being a weak electrolyte in solution is its molecular form. So we don't do not separate the weak acid into its ions. We leave it together well then get soluble calcium acetate. When calcium acetate will produce one calcium ion and two acetate and ions. And then we'll get our two waters. This will be the complete or the total ionic equation. To go from the total ionic equation to the net ionic equation, we need to cancel the spectator ions. The spectator ions are the ions that are common to both sides. In this case it's just calcium. So when the calcium ions are eliminated, then what is left is the net ionic equation to acetic acids react with two hydroxide producing to assist states and two waters. Or we could say just want to see the kassid dividing everything by two reacts with one hydroxide producing one acetate and one water. This is the molecular equation, the total ionic equation and the net ionic equation for the next one, we have phosphoric acid reacting with calcium chloride. This is not a acid base reaction, although phosphoric acid is an acid, this is not a base. But what will happen is the cat ions will switch places and in the process will get calcium going with phosphate and hydrogen going with chloride. When we do that, we end up forming calcium, phosphate, calcium with a two plus charge and phosphate with a three minus charge will require three calcium and to phosphates to get a neutral ionic compound. Then we need to look up the soluble itty rules for calcium phosphate. Is this a solid or is this soluble? And it turns out that it is a solid? It's insoluble. And then the next product will be hydrogen combining with chloride. Each has a a charge of one H one plus chlorine is one minus. So we just need one of each of them. But now we need to balance it. We have three calcium, one calcium, we have two phosphates, one phosphate. So we're going to need to put a two in front of the phosphoric acid and a three in front of the calcium chloride. That then gives us six calcium and six hydrogen. So we need to put a six in front of the hcl al It's separate everything that is soluble into its corresponding species because phosphoric acid is a weak acid, just like acetate. Up here, it's best representation is its molecular form, not its ionic form. Yes, a few hydrogen is come off producing hydrogen ion and di hydrogen phosphate, but most of the molecule stays together, so it's best representation is its molecular forum, calcium chloride, however, is completely soluble, so it's going to separate into three calcium and six chlorides. Then calcium phosphate is insoluble, so it stays together as a solid and then hydrochloric acid is a strong acid, so it does completely separate into six hydrogen ions and six chloride and ions. So we then identify our spectator ions. Just the chlorides are common to both sides, removing the spectator ions gives us our net ionic equation where three calcium ions, combined with two phosphoric acid molecules producing one calcium phosphate species and six hydrogen ions. This is the molecular, the total ionic and the net ionic equation

We have video lessons for 98.09% of the questions in this textbook