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A 25.0 ml of 0.106M KIO3 is put into a 250 ml flask and is titrated to a stoichiometric point with 16.25 ml of a sodium thiosulfate solutiom What Molarity of sodium thiosulfate?
Wiki User
∙ 13y ago
Jodate: IO3- + 6e- + 6H+ --> I- + 3H2O
equivalency to:
Thio: 6S2O32- --> 3S4O62- + 6e-
25.0 ml * 0.106 mmol/ml (KIO3) = 2.65 mmol KIO3 reacting (1:6) with Thio: 6*2.65 = 15.9 mmol sodium thiosulfate. This is in 16.25 ml, so the molarity is 15.9 mmol / 16.25 =
= 0.978 M thiosulfate
Wiki User
∙ 13y ago
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Would your calculated molarity of NaOH be too high too low or unaffected if you titrated to a dark pink color?
it will increase the molarity of the acetic acid
How many moles of sodium hydroxide are used for the tiltration if 17.65 mL of a 0.110 M sodium is needed to titrated 25.00 mL of a hydrochloride acid solution?
I need to see the balanced equation to work!NaOH + HCl --> NaCl + H2O ( good, all one to one )Now, find molarity HCl ( sodium, or sodium hydroxide; no matter )(17.65 mL)(0.110 M NaOH) = (25.00 mL)(X M HCl)= 0.07766 M HCl-------------------------now,Molarity = moles of solute/Liters of solution ( 25.00 mL = 0.025 L)0.07766 M HCl = X moles/0.025 Liters= 0.001942 moles HCl---------------------------------------formal set up, though not needed0.001942 moles HCl (1 mole NaOH/1 mole HCl)= 0.00194 moles sodium hydroxide used=============================
A certain amount of hydrogen peroxide was dissolved in 100 ml of water and then titrated with 1.68m kmno4 how much h2o2 was dissolved if the titration required 22.3 ml of the kmno4 solution?
Mass of H2O2 = 0.637 g
Why is sodium thiosulphate not suitable for use as a primary standard?
Sodium hydroxide cannot be used as a primary standard because of its hygroscopic properties as a solid. Because it is so prone to absorbing water, it is impossible to accurately measure the mass of a solid sample, so instead it must be put into solution and titrated with a known acidic solution. This makes it a secondary standard as opposed to a primary standard. The same logic holds true for hydrated sodium carbonate. Any solution that MUST be titrated in order to know it true molarity is considered a secondary standard. It also reacts with atmospheric carbon dioxide to form sodium carbonate, so it is unstable.
Why hydrogen peroxide was not heated before titrated with potassium permanganate?
Well the question is not very specific, but I think you may be reffering to the boiling of water before acid-base titrations. Water is boiled previous to acid-base titrations because if left open to the atmosphere @ STP water will absorb carbon dioxide until the pH is roughly 5.5. This will obviously adversly affect the accuracy of an acid-base titration. In the permanganate titration, a redox reaction occurs in the presence of an acidic solution.
What does completely titrated mean?
Completely titrated means it reached the stoichiometric point (usually pH=7). Simply means neutralized.
What is the molarity of an naoh solution if 4.37ml is titrated by 11.1 ml of 0.0904 m hno3?
0.289 Moles is the molarity of an NaOH solution if 4.37 ml is titrated by 11.1 ml of 0.0904m hno3.
A 25.0 ml sample of hcl was titrated to the endpoint with 15.0 ml of 2.0 normality naoh what was the normality of th hcl what was its molarity?
The HCL concentration is 1.2M or 1.2N
What is the molarity of an unknown acid if 40.5 ml of the acid can be titrated to an end point by 20.5 ml of .2250 M NaOH?
0.114 M
Why KI is added in redox iodometric titration even in the presence of sodium thiosulfate as a reducing agent?
In iodometric titrations sodium thiosulfate is the titrant whereas the KI will reduce the analyte; eg: Cu2+ to Cu+. The I2 produced is then titrated by the sodium thiosulphate. Cu2+ + I- --> CuI + I3- I3- + 2 S2O32- ¾® 3 I- + S4O62- To answer your question: KI (reducing agent) is added to generate the iodine by the reduction of the analyte (Cu2+) The formed iodine is then back-titrated with thiosulfate (titrant) to determine the amount of analyte originally present. As you can see the KI and sodium thiosulfate serve two different purposes. KI improves solubility of Iodine
Would your calculated molarity of NaOH be too high too low or unaffected if you titrated to a dark pink color?
it will increase the molarity of the acetic acid
A volume of 40.0g of aqueous potassium hydroxide was titrated against a standard solution of sulfuric acid. What was the molarity of the solution if 25.7g of 1.50M was needed?
M = n ÷ V M-Molarity (mol/l) n- moles V- volume in liters. Volume cannot be expressed in grams....
How many moles of Na2S2O3 react with one mole of KClO3 used in the standardization?
Standardization of sodium thiosulfate uses potassium iodate with excess potassium iodide and acidified. Iodine is liberated and that is titrated with sodium thiosulfate. KIO3 + 5KI + 3H2SO4 -----> 3K2SO4 + 3H2O + 3 I2 I2 + 2Na2S2O3 -------> 2NaI + Na2S4O6 So 1 mole of KIO3 produces 3 moles of Iodine. 1 moles of iodine reacts with 2 moles of thiosulfate. So 6 moles of sodium thiosulfate react with 1 mole of potassium iodate KIO3.
Can 2 metals be titrated?
Cations can be titrated.
Given that 31.6ml of 0.141M Na2S2O3 is needed to reach the stoichiometric point how many grams of Cl2 are in the titrated?
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
What is the principle of BOD?
when magnesium sulfate and potassium hydroxide is added,magnesium hydroxide is formed and precipitates and conc H2SO4 is added and in presence of oxygen the preciptate turns brown color which can be measured by idoine and starch indicator titrated against sodium thiosulfate
Can oxalic acid be titrated by HCl?
No; acids can be titrated with bases.
