Question
In: Chemistry
A 7.81 g sample of an aqueous solution of nitric acid contains an unknown amount of...
A 7.81 g sample of an aqueous solution of
nitric acid contains an unknown amount of the
acid.
If 23.2 mL of 1.68 M
potassium hydroxide are required to neutralize the
nitric acid, what is the percent by mass of
nitric acid in the mixture?
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
A 9.15 g sample of an aqueous solution of hydroiodic acid contains an unknown amount of...
A 9.15 g sample of an aqueous solution of hydroiodic acid
contains an unknown amount of the acid. If 29.3 mL of 0.506 M
sodium hydroxide are required to neutralize the hydroiodic acid,
what is the percent by mass of hydroiodic acid in the mixture?
20. An aqueous solution of nitric acid is standardized by titration with a 0.162 M solution...
20. An aqueous solution of nitric acid is standardized by
titration with a 0.162 M solution of potassium hydroxide. If 27.1
mL of base are required to neutralize 20.7 mL of the acid, what is
the molarity of the nitric acid solution? M nitric acid
A solution of an unknown acid is prepared by dissolving 0.250 g of the unknown in...
A solution of an unknown acid is prepared by dissolving 0.250 g
of the unknown in water to produce a total volume of 100.0 mL. Half
of this solution is titrated to a phenolphthalein endpoint,
requiring 12.2 mL of 0.0988 M KOH solution. The titrated solution
is re-combined with the other half of the un-titrated acid and the
pH of the resulting solution is measured to be 4.02. What is are
the Ka value for the acid and the molar...
An aqueous solution containing 15.9 g of an unknown molecular (nonelectrolyte) compound in 106.5 g of...
An aqueous solution containing 15.9 g of an unknown molecular
(nonelectrolyte) compound in 106.5 g of water was found to have a
freezing point of -2.0 ∘C.
Calculate the molar mass of the unknown compound.
The following sequence of reactions occurs in the commercial production of aqueous nitric acid. 4 NH3(g)...
The following sequence of reactions occurs in the commercial
production of aqueous nitric acid. 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6
H2O(l) ΔH = −1166.0 kJ/mol 2 NO(g) + O2(g) → 2 NO2(g) ΔH = −116.2
kJ/mol 3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g) ΔH = −137.3 kJ/mol
Determine the total energy change (in kJ) for the production of one
mole of aqueous nitric acid by this process. _____ kJ
A nitric acid solution is composed of 63.75 g of HNO3 and 205.65 mL of pure...
A nitric acid solution is composed of 63.75 g of HNO3 and 205.65
mL of pure water. What is the percent by mass of the nitric acid
solution? Use the density of water as 0.9984 g/mL.
What are some of the key characteristics of unknown sample of an aqueous solution containing an...
What are some of the key characteristics of unknown sample of an
aqueous solution containing an ionic compound? Specific questions:
1. Given that the cation is from Group 1A, what is the identity of
the group 1A metal ion in your solution? 2. Given that the ionic
compound contains either chloride or hydroxide, how can you
determine which? (Two pieces of evidence are required and one must
be related to solubility rules) 3. What is the concentration of
your solution?...
What are some of the key characteristics of unknown sample of an aqueous solution containing an...
What are some of the key characteristics of unknown sample of an
aqueous solution containing an ionic compound?
Specific questions:
1. Given that the cation is from Group 1A, what is the identity
of the group 1A metal ion in your solution?
2. Given that the ionic compound contains either chloride or
hydroxide, how can you determine which? (Two pieces of evidence are
required and one must be related to solubility rules)
3. What is the concentration of your solution?...
An aqueous solution containing 34.1 g of an unknown molecular (non-electrolyte) compound in 159.9 g of...
An aqueous solution containing 34.1 g of an unknown molecular
(non-electrolyte) compound in 159.9 g of water was found to have a
freezing point of -1.5 ∘ C Calculate the molar mass of the unknown
compound.
A 0.6505 g sample of ferrite ore is dissolved in nitric acid. All of the iron...
A 0.6505 g sample of ferrite ore is dissolved in nitric acid.
All of the iron present is oxidized to iron(III). The solution is
filtered and made basic with addition of ammonium hydroxide. The
iron precipitates as the iron(III) hydroxide hydrated solid. The
precipitate is collected in a crucible and ignited to produce
Fe2O3. What is the mass % of iron in the sample if the analysis
produced 0.3010 g Fe2O3?
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