Liquid-Plumr is a chemical drain opener made of 0.5-2% sodium hydroxide (NaOH, M=40,00 g/mol) and 5-10% sodium hypochlorite (NaClO, M=74.44 g/mol), and a surfactant (detergent, unknown), according to the producer Clorox (to calculate mass% these underscored date are essential)
0.1025(mmol/mL)*(25.25) (mL)*74.44(mg/mmol)*0.001(g/mg) / 3.529(g) * 100% = 5.458% NaClO
(this looks this most reasonable value to me, because the tatration can be done with one buret filling)
However, if 41.58 mL is used to titrate the second part (thus total volume would have been 59.91) then:
0.1025(mmol/mL)*(41.58)(mL)*74.44(mg/mmol)*0.001(g/mg) / 3.529(g) * 100% = 8.988%
(I would advise to use a smaller weight of sample next tim, e.g. about 2 gram LP)
Note: all value were calculated in 4 signifcant digits according to the given figures.
However this does not suggest that the outcomes are as accurate; at least triplicate titrations on 3 different weights (amounts) of the same sample are needed for an accuracy of <0.1% of outcome values.
The equivalence point, also known as the stoichiometric point, of a chemical reaction is when a titrant is added and is stoichiometrically equal to the number of moles of substance, known as analyte, present in the sample: the smallest amount of titrant that is sufficient to fully neutralize the analyte.
First write the balanced chemical equation.HCl (aq) + NaOH (aq) --> NaCl (aq) + H2O (l)Now convert 14.73mL into L by dividing by 1000.14.73 mL * (1L/1000mL) = 0.01473LMultiply the number of liters by the molar concentration of NaOH to get the number of moles in the amount of titrated solution.0.01473L * 0.1025 mol/L = 1.51*10^-3 mol NaOHThe endpoint of the reaction will be approximately the equivalence point, thus at the endpoint:mol HCl = mol NaOHThe coefficient of each reactant should match that of the balanced chemical equation. Both HCl and NaOH have a coefficient of 1 in the balanced chemical equation, thus it is a 1:1 exchange ratio.Now we know that we have reacted equal amounts of HCl and NaOH, so we also know the number of moles of HCl that were reacted in the equation: 1.51*10^-3 molIf we multiply the number of moles of HCl by the molar mass of HCl, we will get the number of grams of HCl present.1.51*10^-3 mol * 36.46 g/mol = 0.0551 g HClNow if we divide the number of grams of HCl present by the total mass of the original sample, we will get the percent by mass of hydrochloric acid in Lysol.0.0551g/0.5725g = 9.62% HCl
Thiosulfate: 2 S2O32- --> S4O62- + 2e-equivalency to:Chlorine: 1 Cl2 + 2e- --> 2Cl-31.6 ml * 0.141 mmol/ml S2O32- = 4.456 mmol S2O32-= 4.456 *(2 electron / 2 S2O32-) = 4.456 mmol (electrons) == 4.456 *(1 Cl2 / 2 electron) = 2.228 mmol Cl2 == 2.228 * 70.90 mg/mmol Cl2 = 158 mg == 0.158 g Chlorine
Cations can be titrated.
No; acids can be titrated with bases.
10.332
an exact volume of the acid is titrated on the base and then placed on a Bunsen burner to be boiled for some time.it can be observed that the salt crystals will be left in the conical flask
titrated
Completely titrated means it reached the stoichiometric point (usually pH=7). Simply means neutralized.
h2c2o2.2h2o
Aqueous titration: the ion to be titrated is in an aqueous solution Nonaqueous titration: the ion to be titrated is in an nonaqueous solution
8.78
methylorange
yes.
8