Group diagnostic acids and bases
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Identify the Bronsted-Lowry acid, Bronsted-Lowry base, conjugate base and conjgate acid from the following equation: NH₄⁺  + H₂O ⇄ NH₃ + H₃O⁺ *
4 points
NH₄⁺
H₂O
NH₃
H₃O⁺
B-L Acid
B-L Base
Conjugate Acid
Conjugate Base
Identify the Bronsted-Lowry acid, Bronsted-Lowry base, conjugate base and conjgate acid from the following equation: HF  + H₂O ⇄ F⁻ + H₃O⁺ *
4 points
HF
H₂O
F⁻
H₃O⁺
B-L Acid
B-L Base
Conjugate Acid
Conjugate Base
Determine the Hydronium ion concentration, the hydroxide ion concentration and the pH of the following solutions:
10 points
0.00112 molL-¹ HCl
0.125 molL-¹ HCl
3.68 x 10⁻² molL-¹ NaOH
0.124 molL-¹ NaOH
pH 0.903
pH 13.1
pH 2.95
pH 12.6
[H₃O⁺] 0.00112 molL-¹  
[H₃O⁺] 0.125 molL-¹  
[OH-] 0.00112 molL-¹  
[OH-] 0.125 molL-¹  
[H₃O⁺] 0.124 molL-¹  
[H₃O⁺]  3.68 x 10⁻² molL-¹  
[OH-]  3.68 x 10⁻² molL-¹  
[OH-] 0.124 molL-¹  
Clear selection
Aqueous solutions of acids HA and HB have the same concentration of 0.100 molL-¹. The pH of HA is 3.5 and HB is 1.8 *
1 point
HA
HB
Which acid is stronger?
Is HA a weak acid or strong acid? *
1 point
Is HB a weakk or strong acid? *
2 points
Aqueous solutions of acids HA and HB have the same concentration of 0.100 molL-¹. The pH of HA is 3.5 and HB is 1.8. Complete the grid *
12 points
HA
HB
[H₃O⁺] 3.16 x 10⁻⁴ molL-¹ 
[H₃O⁺] 1.58 10⁻² molL-¹ 
[OH-] 6.33 10⁻¹³  molL-¹ 
[OH-] 3.16 10⁻¹¹  molL-¹ 
Equilibrium lies further to the right
Equilibrium lies further to the left
More H+ have been donated to water
Less H+ have been donated to water
When Mg is added bubbles of gas are produced more quickly
When Mg is added bubbles of gas are produced, but more slowly
When Mg is added more heat is given off initally
More heat is produced when NaOH is added
Explain the reason for your choice when Mg is added to HA and HB *
0 points
The bicarbonate ion HCO₃⁻ can both accept and donate protons. Complete the equation to show it acting as an acid *
 HCO₃⁻ + H₂O ⇄          
1 point
The bicarbonate ion HCO₃⁻ can both accept and donate protons. Complete the equation to show it acting as a base *
 HCO₃⁻ + H₂O ⇄        
1 point
When sodium bicarboate, NaHCO₃ dissolves in water the solution is basic, Which ion is produced? *
1 point
What is the term used for a compound that both donate and accept protons *
1 point
Methyl Orange can be used as an indicator in acid - base reactions.It is pink in solutions with a pH of less than 3 and yellow in solutions with a pH more than 4. Four beakers contain the following solutions: 0.1 molL-¹  HCl, 0.01 molL-¹ HCl, 0.1  molL-¹ NaOH and distilled water *
Complete the following grid
8 points
0.1 molL-¹ HCl
0.01 molL-¹ HCl
0.1 molL-¹ NaOH
Distilled water
pH = 1
pH = 2
pH = 13
pH = 7
Colour of methyl orange = pink
Colour of methyl orange = yellow
Colour of methyl orange = pink
Colour of methyl orange = yellow
What is the conjugate base of NH₄⁺ *
1 point
Which is the conjugate base of H₂PO₄⁻? *
1 point
Which is the conjugate acid of HSO₄⁻? *
1 point
Write an equation for  HSO₄⁻ acting as an acid. *
1 point
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