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Chemistry
Analytical Chemistry
Titrations and Stoichiometry
A single titration was performed which required 12.60 mL of 0.100 M Na2S2O3. The density of the original, undiluted unknown bleach was 1.040 g/mL. Calculate the number of moles of ClO- in the sample titrated.
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Are you titrating bleach directly with thiosulfate or are you going through an I2 step which you haven't mentioned.
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Suppose a student diluted and titrated a bleach unknown exactly as described in the experimental procedure, except only a single
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(16.22mL) * (1L/1000mL) * (0.100 moles/L) = ? moles
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Suppose a student diluted and titrated a bleach unknown exactly as described in the experimental procedure, except only a single
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Do you have an equation for this. Are you sure you didn't go through an extra step with iodide ion?
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Suppose a student diluted and titrated a bleach unknown exactly as described in the experimental procedure, except only a single
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1. mols = M Na2S2O3 x L Na2S2O3 2. What are you calling reaction 1 and reaction 2? 3,4,5. What is
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Suppose a student diluted and titrated a bleach unknown exactly as described in the experimental procedure, except only a single
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See my question and response above.
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Suppose a student diluted and titrated a bleach unknown. A single titration was performed which required 14.42 mL of 0.100 M
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You're post is too sketchy. For example, did you add KI to the bleach to free up I2 and the I2 was
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Suppose a student diluted and titrated a bleach unknown exactly as described in the experimental procedure, except only a single
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To calculate the number of moles of ClO- in the sample titrated, we need to use the balanced
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single titration was performed which required 11.82 ml of .1 M Na2S2O3
the density of the original undiluted bleach unknown was
Top answer:
Your second equation is not right. It should be I2 + 2[S2O3]^2- ==> [S4O6]^2- + 2I^- 1 mol ClO^- = 1
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Suppose a student diluted and titrated a bleach unknown exactly as described in the experimental procedure, except only a single
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*The density of the original, undiluted bleach unknown was 1.042 g/mL.
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In the titration of Na2S2O3 against KIO3 the average titre value was 23.1cm3,the volume of iodine used in the titration was
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2.34 moles
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I need a balanced chemical equation for the titration of potassium iodate (KIO3^2-) and sodium thiosulfate (Na2S2O3^2-).
This is
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Surely you are confused a little or I just don't know what's going on. Usually something like KI is
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