Strong acids
description
Transcript of Strong acids
![Page 1: Strong acids](https://reader036.fdocuments.us/reader036/viewer/2022081604/56814a71550346895db78a5b/html5/thumbnails/1.jpg)
Strong acids
All (100%) of the H ionize to H+
HCL, H2SO4, HNO3 are all strong acids
![Page 2: Strong acids](https://reader036.fdocuments.us/reader036/viewer/2022081604/56814a71550346895db78a5b/html5/thumbnails/2.jpg)
Strong Bases
All (100%) of the OH ionize to (OH)-
NaOH and KOH are strong bases
![Page 3: Strong acids](https://reader036.fdocuments.us/reader036/viewer/2022081604/56814a71550346895db78a5b/html5/thumbnails/3.jpg)
WEAK acids and bases
Not all the hydrogen ions or hydroxide ions come off (ionize) in solution
Carbonic acid and Phosphoric acids are weak
![Page 4: Strong acids](https://reader036.fdocuments.us/reader036/viewer/2022081604/56814a71550346895db78a5b/html5/thumbnails/4.jpg)
Acid Base Reactions
![Page 5: Strong acids](https://reader036.fdocuments.us/reader036/viewer/2022081604/56814a71550346895db78a5b/html5/thumbnails/5.jpg)
Acids + Metals
In lab we did an experiment with Zinc and acid:
Zn(s) + HCl (aq) H2(g) + ZnCl2 (aq)
Is this equation balanced? Balance it!What type of reaction is it?If we used copper instead of zinc, what would
happen? (hint: look at Table J)
![Page 6: Strong acids](https://reader036.fdocuments.us/reader036/viewer/2022081604/56814a71550346895db78a5b/html5/thumbnails/6.jpg)
Neutralization Reactions
![Page 7: Strong acids](https://reader036.fdocuments.us/reader036/viewer/2022081604/56814a71550346895db78a5b/html5/thumbnails/7.jpg)
Neutralization Reactions
Acid + Base water + a salt
This is true for any acid and base
Because water (pH = 7= neutral) is produced, the acid and the base are neutralized
![Page 8: Strong acids](https://reader036.fdocuments.us/reader036/viewer/2022081604/56814a71550346895db78a5b/html5/thumbnails/8.jpg)
Write Neutralization Reactions for…
Nitric acid + potassium hydroxide
Sulfuric acid + calcium hydroxide
Magnesium hydroxide and hydrochloric acid
![Page 9: Strong acids](https://reader036.fdocuments.us/reader036/viewer/2022081604/56814a71550346895db78a5b/html5/thumbnails/9.jpg)
Titration Equation
Remember: Molarity (M) = Moles/Liter
So…. moles = molarity x Liters
![Page 10: Strong acids](https://reader036.fdocuments.us/reader036/viewer/2022081604/56814a71550346895db78a5b/html5/thumbnails/10.jpg)
Titration Equation
In a neutralization reaction……
the number of moles of acid must be equal to the number of moles of base
(or the end result will not be neutral! )
![Page 11: Strong acids](https://reader036.fdocuments.us/reader036/viewer/2022081604/56814a71550346895db78a5b/html5/thumbnails/11.jpg)
Titration Equation
Therefore, in a neutralization reaction….
Moles of Acid = Moles of Base or Moles (A) = Moles (B)
![Page 12: Strong acids](https://reader036.fdocuments.us/reader036/viewer/2022081604/56814a71550346895db78a5b/html5/thumbnails/12.jpg)
Titration Equation
Since we know that Moles = molarity x Liter,We can substitute in for Moles
Moles of Acid = Moles of BaseMolarity(of acid) x liters(of acid) = Molarity(of base) x Liters
(of base)
![Page 13: Strong acids](https://reader036.fdocuments.us/reader036/viewer/2022081604/56814a71550346895db78a5b/html5/thumbnails/13.jpg)
Titration Equation
We simplify this equation: (see Table T)
Ma x Va = Mb x Vb
Where Ma = molarity of acid Va = volume of acid (in liters) Mb = molarity of base Vb = volume of base (in liters)
![Page 14: Strong acids](https://reader036.fdocuments.us/reader036/viewer/2022081604/56814a71550346895db78a5b/html5/thumbnails/14.jpg)
Ma x Va = Mb x Vb
What is the concentration of HCl if 50 ml of a 0.25M KOH are needed to neutralize 20 ml of HCL solution?
Ma = ?Va = 20 mlMb = .25MVb = 50 ml
Ma x .02L = .25M x .05L
![Page 15: Strong acids](https://reader036.fdocuments.us/reader036/viewer/2022081604/56814a71550346895db78a5b/html5/thumbnails/15.jpg)
Ma x Va = Mb x Vb
What is the concentration of HCl if 50 ml of a 0.25M KOH are needed to neutralize 20 ml of HCL solution?
Ma x .02L = .25M x .05L
Ma = .25M x .05L .02L
Ma = .625M
![Page 16: Strong acids](https://reader036.fdocuments.us/reader036/viewer/2022081604/56814a71550346895db78a5b/html5/thumbnails/16.jpg)
Titration
is used to very accuratelymeasure the volumesof acids and basesduring a neutralizationreaction
Phenolphthalein indicator is clear in acids, pink in bases
![Page 17: Strong acids](https://reader036.fdocuments.us/reader036/viewer/2022081604/56814a71550346895db78a5b/html5/thumbnails/17.jpg)
Neutralization is reachedwhen the clear solution turns a pale pink
![Page 18: Strong acids](https://reader036.fdocuments.us/reader036/viewer/2022081604/56814a71550346895db78a5b/html5/thumbnails/18.jpg)
If solution turns a dark pink, too muchbase has been added and the solution is now basic, not neutral
![Page 19: Strong acids](https://reader036.fdocuments.us/reader036/viewer/2022081604/56814a71550346895db78a5b/html5/thumbnails/19.jpg)
pH
![Page 20: Strong acids](https://reader036.fdocuments.us/reader036/viewer/2022081604/56814a71550346895db78a5b/html5/thumbnails/20.jpg)
pH
• pH = 7 Neutral (pure water)
• pH 0-6 Acidic
• pH 8-14 Basic
![Page 21: Strong acids](https://reader036.fdocuments.us/reader036/viewer/2022081604/56814a71550346895db78a5b/html5/thumbnails/21.jpg)
Indicators: Table M
• Change colors in the presence of acids or bases
• Phenolphthalein = clear in acids, pink in bases
• Litmus = red acid Blue Base