Will a ppt of PBCO3 (s) form if you mix 30 mL of 1.3х 108 М РЫ(NO3)2 (aq) with 120 mL of 5.7 x 10-6 M Na2CO3 (aq)? (Which of the following is entirely correct?) O Q = 7.4 x 10-14, no ppt %3D O = 7.4 x 1014, ppt forms OQ = 2.5 x 10-º, ppt forms OQ = 1.2 x 10-14, ppt forms OQ = 1.2 x 10-14, no ppt

An aqueous ethylene glycol (HOCH₂CH₂OH, FW = 62.07 g/mol) solution with a mass of 214.3 mg is titrated with 61.9 mL of 0.0867 M Cet in 4 M HCIO. The solution is held at 60 °C for 15 min to oxidize the ethylene glycol to formic acid (HCO,H) and carbon dioxide. The excess Cet is titrated with 10.57 mL of 0.0479 M Fe²+ to a ferroin end point. What is the mass percent of ethylene glycol in the unknown solution? mass percent=

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Calculate the percent yield of the experiment

2 HyPOalaq) + 3 Mg(OH)2(ag) = Mga (PO4/21s) + 6 H201 If 35.0 mL of 1.67 M HsPO4 are reacted with 50.0 mL of 1.25 M Mg(OH)2 and 4.892 g of Mg(PO42 (M. W. = 262.86 g/mole) are collected: a) What species is the limiting reagent? b) the theoretical yield of Mg(PO4) in grams ? g c) the percent yield of Mg(PO4)2 ? % d) Whatis thr molarity of excess reagent left over in solution ?

A 0.879 g sample of a CaCl2·2H2O/K2C2O4·H2O solid salt mixture is dissolved in ~100mL of deionized water. The precipitate, after having been filtered and air-dried, has a mass of 0.284 g. The limiting reactant in the salt mixture was later determined to beCaCl2 ·2H2O.   a.Write the ionic equation for the reaction.   b.Write the net ionic equation for the reaction.   c.How many moles and grams of CaCl2 ·2H2O reacted in the reaction mixture?   d.How many moles and grams of the excess reactant, K 2C2O 4H2O, reacted in the mixture?   e.How many grams of the K2C2O4·H2O in the salt mixture remain unreacted (inexcess)?   f.What is the percent by mass of each salt in the mixture

In this experiment, a series of solutions are prepared by combining multiple components into a single container. One solution prepared contains 5.00 mL of (1.1x10^-2) molar KI, 10.00 mL of 0.0010 molar Na2S2O3, 15.00 mL of water, 10.00 mL of (3.90x10^-2) molar KBrO3, and 10.00 mL of (1.000x10^-1) molar HCl. What is the concentration of iodide ions in this solution? Note: Your answer is assumed to be reduced to the highest power possible. When answering this problem, report the answer with the appropriate number of significant figures. Enter your answer USING scientific notation. When entering units, use proper abbreviated units with proper capitalization

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4. In this experiment, ethanol was selected to purify benzoin on Day 1. However, alcohols are inappropriate solvents for recrystallizing compounds containing carboxylic acids. One side reaction is "Esterification" that can occur by placing COOH and OH groups together upon heating. If 3.5 grams of Terephthalic acid and 3 mL methanol undergo esterification, (a) what is the limiting reagent? (b) Predict the grams of the two end products: dimethyl terephthalate and water assuming Esterification is driven to completion. Show calculations. Hint: you can find the grams of methanol through its density.

5. If a 7.0 mL sample of vinegar was titrated to the stoichiometric equivalence point with 7.5 mL of 1.5M NaOH, what is the mass percent of CH₂COOH in the vinegar sample? Show your work. Moles of NaOH used= 1.5M x 7.5 mL = 11.25 millimole Moles of acetic acid in vinegar 11.25 millimole Concentration of acetic acid = 11.25 millimole/7.0 mL = 1.61 M Mass % of acetic acid = 1.61 M x 60 g/mol (molar mass of acetic acid) = 96.43% ????? I