Carbonic acid (H2CO3) is a weak diprotic acid with
Ka1=4.43×10−7 and Ka2=4.73×10−11. When sodium
bicarbonate (NaHCO3) is titrated with hydrochloric acid (HCl), it
acts as a weak base according to the equation
NaHCO3(aq)+HCl(aq)→H2CO3(aq)+NaCl(aq)
Part A
What volume of 0.190 M HCl is required for the complete
neutralization of 1.70 g of NaHCO3 (sodium bicarbonate)?
Express your answer to three significant figures and include the
appropriate units.
Part B
What volume of 0.120 M HCl is required for the complete
neutralization...
Carbonic acid (H2CO3) is a weak diprotic acid with
Ka1=4.43×10−7 and Ka2=4.73×10−11. When sodium
bicarbonate (NaHCO3) is titrated with hydrochloric acid (HCl), it
acts as a weak base according to the equation
NaHCO3(aq)+HCl(aq)→H2CO3(aq)+NaCl(aq)
Suitable indicators are those that change color within the pH
range for the equivalence point of a specific titration. The
expected pH at the equivalence point can be calculated using
pKa values. Suitable indicators for use in titrating
carbonic acid or carbonate solutions are methyl orange and...
Carbonic acid (H2CO3) is a weak diprotic acid with
Ka1=4.43�10?7 and Ka2=4.73�10?11. When sodium
bicarbonate (NaHCO3) is titrated with hydrochloric acid (HCl), it
acts as a weak base according to the equation
NaHCO3(aq)+HCl(aq)?H2CO3(aq)+NaCl(aq)
1)What volume of 0.180M HCl is required for the
complete neutralization of 1.50g of NaHCO3 (sodium
bicarbonate)?
2)What volume of 0.120M HCl is required for the
complete neutralization of 1.10g of Na2CO3 (sodium carbonate)?
3)A sample of NaOH (sodium hydroxide) contains a small amount of
Na2CO3 (sodium...
When Acetic acid (CH3COOH) reacts with sodium
bicarbonate a neutralization reaction occurs: [20 pts]
(a) Write the balanced chemical equation for this reaction.
(b) If you are given 1.26 x 102 g of acetic acid and
1.68 x 102 g of sodium bicarbonate, what reagent would
be limiting?
(c) What would be the theoretical yield of the product(s)?
(d) How many grams of excess reagent would be left over?
(e) If the reaction yielded 68.46 g of the gas, 27.52...
The chemical equation for the reaction of baking soda (sodium
bicarbonate, NaHCO3) and vinegar (acetic acid,
CH3COOH) may be written as two steps. Fill in the
missing information for the chemical equation and balance it. Also
indicate what is the reaction type for each step.
Step 1: ________+ ______ --> CH3COONa
(aq) + H2CO3 (l)
Reaction type:
Step 2: H2CO3 (l) -->
H2O (l) + _________
Reaction type:
When the bromothymol blue (BTB) was exposed to the
CO2...
Write the equation of the carbonic acid bicarbonate buffer system(
you can just use their names since typing chemical formulas can be
difficult) describe the connection between carbon dioxide levels
and hydrogen ion levels and how the respiratory and urinary system
can Compensate when there are various acid/base disorders
1.What hazard is created when an acid is reacted with sodium
bicarbonate? Describe the procedure that you will use to minimize
the hazard posed by the extraction of a carboxylic acid with dilute
aqueous sodium bicarbonate?
2.What does the term, “like dissolves like” mean in the context
of the extraction lab?
3.What type of solution would you use to extract an amine from
an organic phase (e.g. methyl t-butyl ether)?
1.Explain how carbonic acid and bicarbonate are formed in the
blood and the functions they serve.
2. Define the terms acidosis and alkalosis, and explain how they
relate to hypoventilation and hyperventilation.
3. Explain how ventilation is adjusted to help maintain
acid-base balance.
When you add 0.330 g of sodium metal to an excess of
hydrochloric acid, you find that 3430 J of heat are produced. What
is the enthalpy of the reaction as written below?
2Na(s) + 2HCl(aq) ------- 2NaCl(aq) + H2 (g)
Enthalpy of reaction:
Enter your answer in the provided box.
The pH of a bicarbonate-carbonic acid buffer is 7.28.
Calculate the ratio of the concentration of carbonic
acid
(H2CO3) to that of the bicarbonate
ion (HCO3−).
(Ka1 of carbonic acid is 4.2 ×
10−7.)
[H2CO3]
[HCO3−]
=