Give the oxidation number for the species or the indicated atom in the following

Question

Give the oxidation number for the species or the indicated atom in the following: Cs in Cs2O ————— Calculate the mass of KI in grams required to prepare 5.00 × 102 mL of a 3.0 M solution
—————— A sample of 0.3151 g of an ionic compound containing the bromide ion (Br) is dissolved in water and treated with an excess of AgNO3. If the mass of the AgBr precipitate that forms is 0.7199 g, what is the percent by mass of Br in the original compound? ————— A sample of 0.7960 g of an unknown compound containing barium ions (Ba2+) is dissolved in water and treated with an excess of Na2SO4. If the mass of the BaSO4 precipitate formed is 0.7651 g, what is the percent by mass of Ba in the original unknown compound?
—————- How many grams of NaCl are required to precipitate most of the Ag+ ions from 2.50 × 102 mL of 0.0467 M AgNO3 solution?
—————- The concentration of Cu2+ ions in the water (which also contains sulfate ions) discharged from a certain industrial plant is determined by adding excess sodium sulfide (Na2S) solution to 0.600 L of the water. The molecular equation is Na2S(aq) + CuSO4(aq) Na2SO4(aq) + CuS(s)
Calculate the molar concentration of Cu2+ in the water sample if 0.0183 g of solid CuS is formed. ——————— How many grams of KHP are needed to neutralize 75.47 mL of a 0.1041 M NaOH solution? (molar mass of KHP = 204.2 g/mol) ——————— Calculate the volume of a 1.420 M NaOH solution required to titrate 36.75 mL of a 1.500 M H3PO4 solution.
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Give the oxidation number for the species or the indicated atom in the following: Cs in Cs2O ————— Calculate the mass of KI in grams required to prepare 5.00 × 102 mL of a 3.0 M solution
—————— A sample of 0.3151 g of an ionic compound containing the bromide ion (Br) is dissolved in water and treated with an excess of AgNO3. If the mass of the AgBr precipitate that forms is 0.7199 g, what is the percent by mass of Br in the original compound? ————— A sample of 0.7960 g of an unknown compound containing barium ions (Ba2+) is dissolved in water and treated with an excess of Na2SO4. If the mass of the BaSO4 precipitate formed is 0.7651 g, what is the percent by mass of Ba in the original unknown compound?
—————- How many grams of NaCl are required to precipitate most of the Ag+ ions from 2.50 × 102 mL of 0.0467 M AgNO3 solution?
—————- The concentration of Cu2+ ions in the water (which also contains sulfate ions) discharged from a certain industrial plant is determined by adding excess sodium sulfide (Na2S) solution to 0.600 L of the water. The molecular equation is Na2S(aq) + CuSO4(aq) Na2SO4(aq) + CuS(s)
Calculate the molar concentration of Cu2+ in the water sample if 0.0183 g of solid CuS is formed. ——————— How many grams of KHP are needed to neutralize 75.47 mL of a 0.1041 M NaOH solution? (molar mass of KHP = 204.2 g/mol) ——————— Calculate the volume of a 1.420 M NaOH solution required to titrate 36.75 mL of a 1.500 M H3PO4 solution.
—————————
Give the oxidation number for the species or the indicated atom in the following: Cs in Cs2O ————— Calculate the mass of KI in grams required to prepare 5.00 × 102 mL of a 3.0 M solution
—————— A sample of 0.3151 g of an ionic compound containing the bromide ion (Br) is dissolved in water and treated with an excess of AgNO3. If the mass of the AgBr precipitate that forms is 0.7199 g, what is the percent by mass of Br in the original compound? ————— Calculate the mass of KI in grams required to prepare 5.00 × 102 mL of a 3.0 M solution
—————— A sample of 0.3151 g of an ionic compound containing the bromide ion (Br) is dissolved in water and treated with an excess of AgNO3. If the mass of the AgBr precipitate that forms is 0.7199 g, what is the percent by mass of Br in the original compound? A sample of 0.3151 g of an ionic compound containing the bromide ion (Br) is dissolved in water and treated with an excess of AgNO3. If the mass of the AgBr precipitate that forms is 0.7199 g, what is the percent by mass of Br in the original compound? ————— A sample of 0.7960 g of an unknown compound containing barium ions (Ba2+) is dissolved in water and treated with an excess of Na2SO4. If the mass of the BaSO4 precipitate formed is 0.7651 g, what is the percent by mass of Ba in the original unknown compound?
—————- How many grams of NaCl are required to precipitate most of the Ag+ ions from 2.50 × 102 mL of 0.0467 M AgNO3 solution?
—————- The concentration of Cu2+ ions in the water (which also contains sulfate ions) discharged from a certain industrial plant is determined by adding excess sodium sulfide (Na2S) solution to 0.600 L of the water. The molecular equation is Na2S(aq) + CuSO4(aq) Na2SO4(aq) + CuS(s)
Calculate the molar concentration of Cu2+ in the water sample if 0.0183 g of solid CuS is formed. ——————— How many grams of KHP are needed to neutralize 75.47 mL of a 0.1041 M NaOH solution? (molar mass of KHP = 204.2 g/mol) ——————— Calculate the volume of a 1.420 M NaOH solution required to titrate 36.75 mL of a 1.500 M H3PO4 solution.
—————————
The concentration of Cu2+ ions in the water (which also contains sulfate ions) discharged from a certain industrial plant is determined by adding excess sodium sulfide (Na2S) solution to 0.600 L of the water. The molecular equation is Na2S(aq) + CuSO4(aq) Na2SO4(aq) + CuS(s)
Calculate the molar concentration of Cu2+ in the water sample if 0.0183 g of solid CuS is formed. ——————— How many grams of KHP are needed to neutralize 75.47 mL of a 0.1041 M NaOH solution? (molar mass of KHP = 204.2 g/mol) ——————— How many grams of KHP are needed to neutralize 75.47 mL of a 0.1041 M NaOH solution? (molar mass of KHP = 204.2 g/mol) ——————— Calculate the volume of a 1.420 M NaOH solution required to titrate 36.75 mL of a 1.500 M H3PO4 solution.
—————————

Explanation / Answer

1. Cesium Oxide Cs2O, oxygen has an oxidation number of -2, the sum of the oxidation number must be equal to zero, so the Cs2 must have a total oxidation of 2, if we divide it by the coefficient (2) we will get oxidation number of 1

2. Mass of KI, calculate moles of KI

moles = Molarity * Volume = 3 * 5x102 ml = 3 * 500ml = 1500 milimoles of 1.5 moles of KI

now let´s get the molecular weight of KI (internet) 166 g/gmol

mass = moles * molecular weight = 1.5 * 166 = 249 grams

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