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In: Chemistry
Order these chemical species by increasing pH of an 0.1M aqueous solution of each. That is,...
Order these chemical species by increasing pH of an 0.1M aqueous solution of each. That is, imagine making an 0.1M solution of each species. Select 1 next to the species that makes the solution with the lowest pH. Select 2 next to the species that makes the solution with the next higher pH, and so on. Notice that some of the rankings have been filled in for you already. Also notice that water is on the list. For that particular case, just compare the pH of pure water to the pH of the other solutions. Note for advanced students: for all charged species, you may assume the necessary counterions act as neither acids nor bases. species relative pH of 0.1M aqueous solution HF ▼(Choose one) ClO2− ▼(Choose one) HClO2 1 (lowest) H2O 4 NO2− 7 OH− ▼(Choose one) F− 6 HNO2 ▼(Choose one)
Solutions
queen_honey_blossom answered 1 year agoRelated Solutions
Order these chemical species by increasing pH of an 0.1M aqueous solution of each. That is,...
Order these chemical species by increasing pH of an 0.1M aqueous
solution of each. That is, imagine making an 0.1M solution of each
species. Select 1 next to the species that makes the solution with
the lowest pH. Select 2 next to the species that makes the solution
with the next higher pH, and so on. Notice that some of the
rankings have been filled in for you already. Also notice that
water is on the list. For that particular...
Using a pH 10 buffer solution of aqueous ammonia and aqueous ammonium chloride, which chemical species...
Using a pH 10 buffer solution of aqueous ammonia and aqueous
ammonium chloride, which chemical species is the weak base? Which
is the conjugate acid? How do you know?
Arrange the following 0.1M solutions in order of increasing pH and state why you placed each...
Arrange the following 0.1M solutions in order of increasing pH
and state why you placed each solution in that position: NaCH3COO,
HCl, HCN, NaOH, NH3, NaCN, KNO3, H2SO4, NH4Cl, H2SO3, NaHCO3,
Na3PO4, and CH3COOH.
Assuming each solution to be 0.10 M , rank the following aqueous solutions in order of decreasing pH.
Assuming each solution to be 0.10 M, rank the following aqueous solutions in order of decreasing pH.
Rank the solutions from the highest to lowest pH. To rank items as equivalent, overlap them
N2H2
Ba(OH)2
HOCL
NAOH
HCL
You measured the pH of a 0.1M HCl solution. If you had diluted this solution by...
You measured the pH of a 0.1M HCl solution. If you had diluted
this solution by adding 100mL of water, what happens to the
concentration of H3O+?
Sort the following in order of increasing acidity in aqueous solution. Explain your reasoning. (You can...
Sort the following in order of increasing acidity in aqueous
solution. Explain your reasoning. (You can check your results by
finding the pKa, but this will not be considered a valid
explanation).
HCrO4 - HSO4 - HSO3 - HClO4
Sort the following in order of increasing acidity in aqueous solution. Explain your reasoning. (You can...
Sort the following in order of increasing acidity in aqueous
solution. Explain your reasoning. (You can check your results by
finding the pKa, but this will not be considered a valid
explanation).
HCrO4 - HSO4 - HSO3 - HClO4
Indicate how the concentration of each aqueous species in the chemical equation changes to reestablish equilibrium afte...
Indicate how the concentration of each aqueous species in the chemical equation changes to reestablish equilibrium after changing the concentration of a reactant or product. Also indicate how the pH changes. An up arrow indicates an increase in concentration, a down arrow indicates a decrease in concentration, and leaving it blank means there is no change in the concentration. HCN(aq) +H2O(l) ⇌ CN-(aq) + H3O+ (aq) pH after the concentration of HCN is increased after the concentration of CN is decreased
The pH of a white vinegar solution is 2.11. This vinegar is an aqueous solution of...
The pH of a white vinegar solution is 2.11.
This vinegar is an aqueous solution of acetic acid with a density
of 1.09 g/mL. What is the mass percentage of acetic acid in the
solution? Ka (acetic acid)= 1.8 X10-5
Mass percentage =___________ %
The pH of a 0.00125 M solution of an aqueous solution of XOH (X = an...
The pH of a 0.00125 M solution of an aqueous solution of XOH (X
= an unknown element) is 3.55. Is XOH a strong acid, weak acid,
strong base, or weak base? How do you know? Is X a metal or
non-metal? Explain
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