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Double Displacement Reactions: Ionic Equilibria and Solubility Rules, Summaries of Chemistry

Northwestern Oklahoma State University (NWOSU)Chemistry

Instructions on how to write ion pairs for double displacement reactions, make formulas for possible products, balance equations, and predict phase labels. It also includes solubility rules for various ionic compounds, which indicate which compounds are mostly soluble or insoluble in water, and exceptions to these rules.

What you will learn

  • Which ions form mostly soluble compounds when paired with certain ions according to the solubility rules?
  • What is the name of the precipitate formed when lead(II) nitrate and sodium iodide solutions react?
  • What are the steps to write the ion pairs for a double displacement reaction?

Typology: Summaries

2021/2022

Uploaded on 09/12/2022

laskhminaran
laskhminaran 🇺🇸

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bg1
Double displacement reaction
: two ionic reactants swap
their ions
AgNO
3
(
aq
) + NaI(
aq
)
→
Write ion pairs for reactants
1.
Swap ions, make new +/
-
pairs, writing + ion first
2.
Make formulas for possible products from new ion
pairs
3.
Balance if necessary
4.
Predict phase labels of products
5.
Double displacement, solubility, and precipitation
ch7b Page 1
pf3

Partial preview of the text

Download Double Displacement Reactions: Ionic Equilibria and Solubility Rules and more Summaries Chemistry in PDF only on Docsity!

Double displacement reaction: two ionic reactants swap their ions AgNO 3 (aq) + NaI(aq) →

  1. Write ion pairs for reactants
  2. Swap ions, make new +/- pairs, writing + ion first Make formulas for possible products from new ion pairs
  1. Balance if necessary
  2. Predict phase labels of products Double displacement, solubility, and precipitation

Some ionic compounds easily dissolve in water (soluble) Some never dissolve in water (insoluble) Solubility Rules for Ionic Compounds The following table will be given on the exam exactly as shown here. Compounds Containing the Following Ions Are Mostly Soluble Exceptions Li+, Na+, K+, NH 4 +^ None nitrate, acetate None chloride, bromide, iodide When any of these ions pairs with Ag+, Hg 2 2+, or Pb2+, the compound is insoluble sulfate When sulfate pairs with Sr2+, Ba2+, Pb2+, or Ca2+^ the compound is insoluble Compounds Containing the Following Ions Are Mostly Insoluble Exceptions hydroxide, sulfide When either of these ions pairs with Li+, Na+, K+, or NH 4 +, the compound is soluble When sulfide pairs with Ca2+, Sr2+, or Ba2+, the compound is soluble When hydroxide pairs with Ca2+, Sr2+, or Ba2+, the compound is slightly soluble (for many purposes, these may be considered insoluble) carbonate, phosphate When either of these ions pairs with Li+, Na+, K+, or NH 4 +, the compound is soluble Na 3 PO 4 Ca 3 (PO 4 ) 2 CaI PbI 2 Fe(OH) 3 Ca(OH) 2 K 2 CO 3 CuCO 3 Solubility of ionic compounds