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A molecule is found to contain 47.35% by mass C, 10.60% by mass H, and 42.05% by mass O. What is the empirical formula for this molecule? Please show step by step how you got this.
Assuming stomach acid is 0.1 M HCl, how many grams of stomach acid would have been neutralized by311mg of Mg(OH)2
A titration was performed between 25 mL of 0.100 M NH3 and 0.100 M HCl. Calculate the pH of NH3 solution at the following points during the titration.
which is to say that potassium iodide is added to the sodium chloride as a nutrient. When a 4.2962 g sample of table salt was analyzed by precipitating the halides with silver nitrate, 10.4192 g of a miture of AgCl and AgI resulted.
Explain when 2-methylpropanoyl chloride reacts with 3-methylbutanoic acid in the presence of the weak base, pyridine. Depict the tetrahedral intermediate where all atoms have a zero formal charge.
Consider the reaction with the rate law, Rate = k[BrO3-][Br-][H+]2 By what factor does the rate change if the concentration of H+ is decreased by a factor of 3
Determine the ratio of HCO3- to H2CO3 in the patient's blood at this pH. Next, consider a normal blood pH of 7.4. How does this ratio compared to the ratio of HCO3- to H2CO3 in normal blood
Alkynes have the general molecular formula CnH2n-2. Thus, when n = 2, the alkyne is C2H2, etc. If an alkyne has a molecular mass between 75 and 85, this alkyne is
How many mL of 0.145 M NaOH solution will be required to neutralize 5.00 mL of a 0.829 M HCl solution
Calculate the heat required to convert 24.0 g of C2Cl3F3 from a liquid at 12.00°C to a gas at 56.00°C
Calculate the percentage yield if 0.2 moles of H2O was formed when 0.6 mol of methane
calculate the alkaline strength of a sample of impure k2co3 in terms of per cent k2o from the following data wt. of
A student followed the procedure of this experiment to determine the Caloric content of a Planter's cocktail peanut. The peanut studied had a mass of 0.609 g before combustion and 0.053 g after combustion
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