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A 1.00 mL sample of dilute acetic acid required 23.4 mL of 0.10 M sodium hydroxide solution to titrate the sample to a phenolphthalein endpoint (which is assumed to be close in pH to the equivalence point). What was the concentration of acetic acid in the sample (show your work)? How many significant figures are justified in your answer? Why?
Suppose that you have 0.500 L of each of the following solutions, and an unlimited supply of water. (Note: C9H7NHBr is a salt containing the ions C9H7NH+ and Br- and C9H7N is quinoline
What weight of malononitrile would be recovered by extraction with (a) three 100-mL portions of ether; (b) one 300-mL portion of ether.
The reaction of combustion of ethanol is this: C2H5OH(g) +3O2(g) ---> 2CO2(g) + 3H2O (g) Los regalitos son ( g ) Lis 4 tienen(g ) A) calculate delta H of the reaction in kj/mol
The oxide of which of the following metals should have the greatest lattice energy?
Why is it that when you look into any type of light for a long period of time that blotches of black appear when you look away
what is the acid dissociation constant of a weak acid if a concentration of 0.3 M gives a hydrogen ion concentration of 0.001M?
The following reaction is for solvolysis of t-butyl chloride. Show mechanism for the formation of the major and minor products. (CH3)3CCl + H2O--------(CH3)3COH+(CH3)2=CH2
The bonding in BF3 requires formation of hybrid orbitals on boron. If the molecule is oriented in the xy plane, what is the identity of the unfilled p orbital on boron.
The isotope 22Na has a half-life of 2.60 years. How much of a 1.00 gram sample would be left after 1.00 yr
What ions and/or molecules are present in relatively large proportions in a solution of a soluble ionic compound NaCl (aq)
You have 493 mL of chlorine trifluoride gas at 699mmHg and 45 degrees Celsius. What is the mass (in grams) of the sample.
Suppose a reaction has a standard Gibbs-free energy of 2.20 kJ/mol, calculate the relative ratio of product to reactant.
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