Question
In: Chemistry
A lab student has made a hydrochloric acid solution which they need to standardize using sodium...
A lab student has made a hydrochloric acid solution which they need to standardize using sodium carbonate (Na2CO3). The concentration of the hydrochloric acid solution is believed to be 0.117 M. The lab student would like the titration to take a volume of 30 mL. What mass of sodium carbonate should the student weigh out for this titration
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
An acetic acid/ sodium acetate buffer solution similar to the one you made in the lab...
An acetic acid/ sodium acetate buffer solution similar to the
one you made in the lab was prepared using the following
components:
3.46 g of
NaC2H3O2∙3H2O (FW. 136
g/mol)
9.0 mL of 3.0 M HC2H3O2
55.0 mL of water
If you take half of this solution and add 2 mL of 1.00 M NaOH to
it, then what is the pH of this new solution?
An acetic acid/ sodium acetate buffer solution similar to the one you made in the lab...
An acetic acid/ sodium acetate buffer solution similar to the
one you made in the lab was prepared using the following
components: 3.46 g of NaC2H3O2∙3H2O (FW. 136 g/mol) 9.0 mL of 3.0 M
HC2H3O2 55.0 mL of water If you take half of this solution and add
2 mL of 1.00 M HCl to it, then what is the pH of this new
solution?
An acetic acid/ sodium acetate buffer solution similar to the one you made in the lab...
An acetic acid/ sodium acetate buffer solution similar to the
one you made in the lab was prepared using the following
components: 3.46 g of NaC2H3O2∙3H2O (FW. 136 g/mol) 9.0 mL of 3.0 M
HC2H3O2 55.0 mL of water If you take half of this solution and add
2 mL of 1.00 M HCl to it, then what is the pH of this new
solution?
A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weights out...
A chemistry student needs to standardize a fresh solution of
sodium hydroxide. She carefully weights out 305.mg of oxalic
acid(H2C2O4), a diprotic acid that can be purchased inexpensively
in high purity, and dissolves it in 250.mL of distilled water. The
student then titrates the oxalic acid solution with her sodium
hydroxide solution. When the titration reaches the equivalence
point, the student finds she has used 69.4mL of sodium hydroxide
solution. Calculate the molarity of the student's sodium hydroxide
solution. Be...
Ethanol reacts with sodium dichromate in an aqueous hydrochloric acid solution according to the balanced net...
Ethanol reacts with sodium dichromate in an aqueous hydrochloric
acid solution according to the balanced net ionic equation shown
below.
3 C2H5OH (aq) + 2
Cr2O72- (aq) + 16 H+
(aq) → 3 HC2H3O2 (aq) + 4
Cr3+ (aq) + 11 H2O (l)
This reaction is carried out with 1.00 mL of
C2H5OH (density 0.816 g/mL, molar mass 46.07
g/mole) reacting with 32.76 mL of a solution that is 0.5775 M in
Na2Cr2O7 and 6.000 M in HCl.
What is...
how is hydrochloric acid made in the stomach?
how is hydrochloric acid made in the stomach?
Sodium cyanide solution, when poured into excess hydrochloric acid, releases hydrogen cyanide as a gas. The...
Sodium cyanide solution, when poured into excess hydrochloric
acid, releases hydrogen cyanide as a gas. The reaction is NaCN(aq)
+ HCl(aq) → HCN(g) + NaCl(aq) Identify the conjugate acid–base
pairs in this reaction out of the following. HCN and Cl- HCN and
CN- CN- and HCl HCl and Cl–
Calculate the molarity of a solution made by adding 25.4 mL of concentrated hydrochloric acid (37.3...
Calculate the molarity of a solution made by adding 25.4 mL of
concentrated hydrochloric acid (37.3 % by mass, density 1.19 g/mL)
to some water in a volumetric flask, then adding water to the mark
to make exactly 500 mL of solution. (It is important to add
concentrated acid or base to water, rather than the other way, to
minimize splashing and maximize safety.)
A 22.26-mL sample of hydrochloric acid solution requires 35.00 mL of 0.115 M sodium hydroxide for...
A 22.26-mL sample of hydrochloric acid solution requires 35.00
mL of 0.115 M sodium hydroxide for complete neutralization. What is
the concentration of the original hydrochloric acid solution?
The concentration of hydrochloric acid can be measured by reacting the acid with pure sodium carbonate....
The concentration of hydrochloric acid can be measured by
reacting the acid with pure sodium carbonate.
a) Write the balanced chemical equation for this reaction.
b) If the complete reaction with 0.8642 (±0.0005) g of sodium
carbonate (FW= 105.9884 ±0.0007) required 42.36 (±0.04) mL of acid,
what is the molarity of the acid. Report the value with its
absolute uncertainty.
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