"Under titration" refers to cases when the equivalence point is not reached, which means that the amount of titrant added is lower than it should have been. This problems leads to errors by defect, in which the calculated concentration of the compound being titrated is lower than the real one. If we are titrating magnesium hydroxide, what we are doing is titrating the OH- with an acid. If we under-titrated, we would obtain a concentration value for OH- that is lower than the real concentration in the sample. Which means that, when we write the empirical formula of the compound, we will have a defect in (OH); that is: there will be less than there should be.
how would under titration affect the empirical formula of magnesuim hydroxide
How would the following errors affect the empirical formula of the compound for a hypothetical student performing s experiment? Note: Writing the answer will be incorrect is not sufficient for these questions. This student is not E) you nor is their data assumed to be the same as yours. student ran out of time and did not do the second heating. Explain thoroughly how this error will affect the water in the hydrate? Will the moles of water calculated be...
In the Titration Lab, how would it affect your results if you used a beaker with residual water in it to measure out your standardized sodium hydroxide solution?
I specifically need help with the last question asking about how this would affect the molecular formula, thank you 4. If some of the calcium metal remains unreacted when you start the titration, the calcium will react with hydrochloric acid to produce hydrogen gas. Ca (s) + 2 HCl(aq) + CaCl, (aq) + H, (g) Would this cause error in the titration? If so, would more or less HCl be required? How would this affect the molecular formula for calcium...
1. How would using double the volume of hydrochloric acid have affected the empirical formula of zinc chloride? 2. Suppose that you had not driven off all the water from the zinc chloride. How would this error have affected the empirical formula for zinc chloride?
Lab #19; Empirical Formula of Magnesium Hydroxide Pre-Lab Questions Name: Heating 1.29 g of gallium gives a gallium-oxygen compound with a mass of 1.739 Calculate the empirical formula of the compound. Step 1: Figure out how many grams of oxygen are in the 1.73 grams of gallium-oxygen compound. Step 2: Convert the 1.29 g of gallium to moles: Step 3: Convert the grams of oxygen you calculated in step 1 to moles: Step 4: Figure out the formula. Formula Name
Determine whether each chemical formula given is an empirical formula or not. Empirical formula Not empirical formula Answer Bank G CH P P PF (co, CO2 NaCl Naci) Col. C,H,O, 10 about us careers privacy policy terms of use contact us help
1. How would using double the volume of hydrochloric acid have affected the empirical formula of zinc chloride? 2. Suppose that you had not driven off all the water from the zinc chloride. How would this error have affected the empirical formula for zinc chloride?
Determine the empirical formula for the compound with the molecular formula B,CI. empirical formula: Determine the empiricalformula for the compound with the molecular formula N, B, H, empirical formula:
What would be the empirical formula for a substance that contains 84.98% by mass Hg and 15.02% by mass Cl? If the molar mass of the substance is 472.1 g/mol what is the molecular formula?
what is the empirical formula for Al2(SO4)3 What is the empirical formula for C6H10