How many mL of 0.250 M KMnO4 are needed to react with 3.55 g of Iron...
How many mL of 0.265 M KMnO4 solution are needed to react with 4.42 g of iron (II) sulfate? 2 KMnO4 + 10 FeSO4 + 8 H2SO4 –> 5 Fe2(SO4)3 + 2 MnSO4 + K2SO4 + 8 H2O
4. How many mL of 0.250 M KM O4 are needed to react with 3.36 g of FeSO4? 10 FESO4 + 2 KMnO4 +8 H2SO4-5 Fe2 (SO4)3 +2 MnSO4 +8H20 +K2SO4 5. Potassium chlorate reacts with hydrochloric acid to produce chlorine gas. What mass of KCIO3 is needed to make 4.50 L of chlorine at 2.35 atm and 37.0°C? KCIO3(g)+6HCI(aq) KCI(aq) + 3C12(g) + 3H2O(1)
WOL 2. What volume of 0.250 M HCl is required to completely react with 0.350 g of Na2CO3? Na2CO3(s) + 2HCl(aq) + 2NaCl(aq) + H2O(l) + CO2(g) 3. Calcium carbonate decomposes at high temperatures to give calcium oxide carbon dioxide. What volume of CO2 will be collected at 950 torr and 500°C when 75.0 g of CaCO3 react? CaCO3(s) → Cao(s) + CO2(g) 4. How many mL of 0.250 M KMnO4 are needed to react with 3.36 g of FeSO4...
Part A A volume of 70.0 mL of aqueous potassium hydroxide (KOH) was titrated against a standard solution of sulfuric acid (H2SO4). What was the molarity of the KOH solution if 25.7 mL of 1.50 M H2SO4 was needed? The equation is 2KOH(aq)+H2SO4(aq)→K2SO4(aq)+2H2O(l) Part B Redox titrations are used to determine the amounts of oxidizing and reducing agents in solution. For example, a solution of hydrogen peroxide, H2O2, can be titrated against a solution of potassium permanganate, KMnO4. The following...
QUESTION 1: A volume of 80.0 mL of aqueous potassium hydroxide (KOH) was titrated against a standard solution of sulfuric acid (H2SO4). What was the molarity of the KOH solution if 12.2 mL of 1.50 M H2SO4 was needed? The equation is 2KOH(aq)+H2SO4(aq)→K2SO4(aq)+2H2O(l) QUESTION 2: Redox titrations are used to determine the amounts of oxidizing and reducing agents in solution. For example, a solution of hydrogen peroxide, H2O2, can be titrated against a solution of potassium permanganate, KMnO4. The following...
A volume of 70.0 mL of aqueous potassium hydroxide (KOH) was titrated against a standard solution of sulfuric acid (H2SO4). What was the molarity of the KOH solution if 15.2 mL of 1.50 M H2SO4 was needed? The equation is 2KOH(aq)+H2SO4(aq)?K2SO4(aq)+2H2O(l) part b: Redox titrations are used to determine the amounts of oxidizing and reducing agents in solution. For example, a solution of hydrogen peroxide, H2O2, can be titrated against a solution of potassium permanganate, KMnO4. The following equation represents...
Part A A volume of 70.0 mL of aqueous potassium hydroxide (KOH) was titrated against a standard solution of sulfuric acid (H2SO4). What was the molarity of the KOH solution if 19.7 mL of 1.50 M H2SO4 was needed? The equation is 2KOH(aq)+H2SO4(aq)→K2SO4(aq)+2H2O(l) Express your answer with the appropriate units. Part B Redox titrations are used to determine the amounts of oxidizing and reducing agents in solution. For example, a solution of hydrogen peroxide, H2O2, can be titrated against a...
How many mL of 0.300 M AlCl3 react with exactly 20.0 mL of 0.250 M Na2SO4(aq) given the reaction: 2 AlCl3 + 3 Na2SO4 -> Al2(SO4)3 + 6 NaCl A. 11.1 mL B. None of these choices is correct C. 1.00 mL D. 16.7 mL E. 25.0 mL
How many milliliters of 0.250 M FeCl3 are needed to react with an excess of Na2S to produce 3.50 g of Fe2S3 if the percent yield for the reaction is 70.0%? 3 Na2S(aq) + 2 FeCl3(aq) ? Fe2S3(s) + 6 NaCl(aq)
How many grams of NaH2PO4 are needed to react with 71.11 mL of 0.881 M NaOH? NaH2PO4(s) + 2NaOH(aq) → Na3PO4(aq) + 2H2O(l)