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17.6 Finding the -- Part 1
Bases are solutions that produce OH- in solution or accept protons.
Bases can be strong or weak in the same way acids can be strong or weak.
The table shows the strong bases for a 1.0 M NaOH solution.
When NaOH is dissolved in water, it forms Na+.
The solution doesn't contain anything.
The strongest bases are group 1A or group 2A metal hydrox.
The group 1A metal hydroxides can form trated base solutions.
The general formula for the group 2A metal hydroxides Calcium hydroxide is M(OH)2.
They produce 2 mol of OH when they are dissolved in water.
There will be 6 1.0 M in a 1.0 M NH3 solution.
NH 3 can partially ionize in water.
There is a complete table in Appendix IIC.
All but two of the weak bases listed in Table 17.8 are ammonia or an amine, which we can think of as ammonia with one or more hydrocarbon groups substituting for one or more hydrogen atoms.
There is a nitrogen atom with a lone pair in all of these bases.
A positively charged ion such as Na+ is needed to balance the charge, but it does not have any part in the ionization reaction.
It is the bicarbonate ion that makes NaHCO3 basic.
Section 17.8 contains ionic bases.
Weak bases have a nitrogen atom with a single pair of protons.
As we did in calculating the H3O+ in strong acid solutions, we can neglect the contribution of the autoionization of water to the OH- and focus solely on the strong base.
Determine the OH- concentration in each solution.
The concentration of OH- is the same as the concentration of KOH.
Substitute [H3O+] into the expression to find the pH.
Substitute H3O+ into the expression to find the pH.
We neglect the contribution of the autoionization of water to the weak base.
To find the contribution of the weak base, we need to prepare an ICE table showing the relevant concentrations of all species and then use the base ionized constant expression to find the OH-.
The expressions for the equilibrium concentrations should be replaced with the expression for the base ionization constant.
The ratio should be less than 5%.
The approximation is valid.
Substitute H3O+ into the equation.
The active ingredients of a heterogeneous mixture of antacids include the following: which the solid is finely divided into the liquid.
Amphogel Al(OH)3 was compared to a group 1A metal hydroxide.
There is excess stomach acid.
There are three main groups of antacids: calcium, magnesium and aluminum.
It would seem as though a quick return of the concentration would make the antacid less effective.
Solid magnesium and aluminum-based antacids can cause acid rebound, but they have drawbacks.
For example, a suspension of aluminum-based antacids tend to cause snoozing and a suspension of magnesium-based ones tend to cause snoozing.
As stomach acid is neutralized, OH- is used up, and the Notice shows the absence of group 1A metal hydroxides, such as KOH equilibrium shifts to the right.
A suspension of Mg(OH)2 provides a steady concentration of are completelysoluble and act as strong bases, not used in dissolved OH- ion to neutralize stomach acid.
The mouth and throat would burn if a solution with enough KOH or NaOH was used.
Some ion act as bases.
The salt of bicarbonate is called sodium bicarbonate.
The sodium ion does not ionize water and has neither acidic nor basic properties.
The weak base of the bicarbonate ion is shown to form a basic solution.
The solution is basic and the pH is above 7.
Some of the acid base properties of salts are considered in this section.
When put into water, some salts are acidic while others are basic.
The conjugate base of an acid is anion.
The conjugate base of the acid HA is the anion A-.
Every anion can potentially act as a base since it is the conjugate base of an acid.
It depends on the strength of the acid.
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