A volume of 25.00mL of a manganese(II) solujtion is titrated in basic conditions with a volume of 34.77mL of 0.05876 M KMnO4. Determine the concentration of manganese(II) ions in the solution.
Mn^2+(aq) + KMnO4^-(aq)--->MnO2(s) (unbalanced)
A volume of 25.00mL of a manganese(II) solujtion is titrated in basic conditions with a volume...
• CIU TEXAS INSTRUM 2. A 50.00 ml sample of solution containing Fe?ions is titrated with a 0.0216 M KMnO4 solution. It required 20.62 ml of the KMnO4 solution to oxidize all the Fe? ions to Fe ions by the reaction: MnO4 (aq) + Fe? ) -------> Mn(ed) Felco (unbalanced) a) What was the concentration of Fel.ions in the sample solution? b) What volume of 0.0150 M K2Cr2O7 solution would it take to do the same titration? The reaction is:...
An acidic solution of potassium permanganate reacts with oxalate ions to form co2 and manganese(II) ions according to the following unbalanced REDOX equation: MnO4-(aq)+C2O4 ^ (2-) --> CO2(G) + Mn ^ (2+) In the banalced equation the coefficients for MnO4- and CO2 is?
In an acidic solution, permanganate ion reacts with tin(II) ion to give manganese(II) lon and tin(IV) ion. (a) Enter a balanced net ionic equation for the reaction (include physical states in your answer). 2+ 2+ 4+ 2MnO& (aq) + 5Sn (aq)+16H (aq)-2Mn (aq) + 5Sn (ag)+8H O) Save & Close Undo Select Erase Help 7 8 (aq) (g) () (s) 4 5 6 e + E NONE 1 2 C F NR Na Mg Al Si P CI K Ca...
18) When an aqueous solution of manganese (ll) nitrate is combined with an aqueous solution of ammonium sulfide, what should precipitate out? A) Mns B) Mn(SO3)2 C) Mn(SO4)2 D) Mn 2503 E) Mn 2504 19) If 4.89 g of ZnCl2 is dissolved in enough water to give a total volume of 500 ml, what is the molarity of the solution? A) 0.217M B) 0.0179 M C) 0.0717 M D) 1.33 M E) 0.849 M 20) What element is undergoing oxidation...
When the following reaction is balanced under basic conditions, what is the ratio of the coefficients of Mn(OH)2(s) to MnO4--(aq)? Mn(OH)2(s) + MnO4 (aq) + MnO42-(aq) (A) 3:1 (B) 1:3 (C) 1:4 (D) 1:5 What is the standard reduction potential for the reduction of permanganate ion to managanese dioxide in acidic solution? Half-Reaction E. V MnO4 (aq) + 8 H(aq) + 5 € → Mn²+ (aq) + +1.51 4 H2O(1) MnO2(s) + 4 H (aq) + 2 e → Mn2+(aq)...
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...
Data Table. Don't forget to include units and show your work for processed data! Raw Data: Initial KMnO, buret reading Final KMnO, buret reading Weight of Fe(NH.)2(SO4)2 Processed Data (show all work for credit): 4.85 ml UL.SIML l ugrams Moles of Fe(NH4)2(50.)zin flask # of electrons donated per Fe(NH4)2(SO4)2 molecule (from balanced half-reaction) Total moles of electrons donated by Fe Total moles of electrons accepted by KMnO4 # of electrons absorbed per KMnO4 (from balanced half-reaction) Moles of KMnO, added...
Part A Manganese reacts with hydrochloric acid to produce manganese(II) chloride and hydrogen gas. Mn(s) + 2 HCl(aq) + MnCl, (aq) + H (9) When 0.620 g Mn is combined with enough hydrochloric acid to make 100.0 mL of solution in a coffee-cup calorimeter, all of the Mn reacts, raising the temperature of the solution from 23.5°C to 28.6 °C. Find AHxn for the reaction as written. (Assume that the specific heat capacity of the solution is 4.18 J/g °C...
What is the molar solubility of manganese sulfide? M What is the concentration of manganese ions in a saturated solution of manganese sulfide? M Manganese Mn(OH)2 1.9 x 10-13 MnCO3 8.8 x 10-11 MnS 5.6 x 10-16
When the following half reaction is balanced under basic conditions, what are the coefficients of the species shown? Но ОН MnO2 Mn(ОН)2 + In the above half reaction, the oxidation state of manganese changes from to