Even in basic solution, Mn04 can oxidize water. One product is manganese(IV)oxide. Write a balanced chemical equation for the reactiona.2MNO4 (aq) + 2H20() ---> 2Mn2+(aq) + 302(g) + 40H (aq)b.4MNO4 (aq) + 2H20() ---> 4MNO2(s) + 302(g) + 40H"(aq)MnO4 (aq) + H20() --> MnO2(s) + H2(g) + OH¯(aq)d.4MNO4 (aq) + H20() ---> 4Mno(s) + O2(g) + 20H (aq)- > MnO2(s) + 2H2(g) + 80H (aq)e.MnO4 (aq) + 6H20(1)市 @Type here to searchC.

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Answered: Even in basic solution, MnO4 can…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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For the balanced reaction Mn2(SO4)5(aq) + 10LiOH(aq) --> 2Mn(OH)5(s) + 5Li2SO4(aq)how many grams of lithium sulfate are produced by this reaction if 148 g of manganese (V) hydroxide are also produced?
If 365 mL of 0.285 M MgCl₂ is added to 235 mL of 0.215 M (NH₄)₃PO₄, how many moles of Mg₃(PO₄)₂ precipitate will be formed? The balanced equation is 3 MgCl₂(aq) + 2 (NH₄)₃PO₄(aq) → Mg₃(PO₄)₂(s) + 6 NH₄Cl((aq)
What is the molarity of Na* ions in a 0.20 M Na2CO3 solution? N22CO3 (s) → 2 Na* (aq) + CO3 2- (aq.
Using the balanced reaction for a solution of aluminum hydroxide reacting with sulfuric acid 2Al(OH)3 (aq) + 3H2SO4(aq) --> Al2(SO4)3 (aq) + 3H2O(l) How many mL of 0.234 M sulfuric acid acid are needed to neutralize an aqueous solution made of 5.987 g of Al(OH)3? MM of Al(OH)3 is 78.004 g/mL
4. Calculate the calculate the mass of precipitate formed from 5.0 g of strontium chloride. Li3PO4(aq) → Sr3(PO4)2(S) + LiCl(aq) _SrCl₂(aq) + 5. What mass of aluminum hydroxide in needed to neutralize 5.00 g of hydrochloric acid? Al(OH)3(s) + _HCl(aq) → ___AlCl3(aq) + _H₂O(1) 195
2. Exactly 23.0 mL of a H₂SO4 solution was required to neutralize 25.0 mL of 0.195 M NaOH. What was the concentration of the H₂SO4 solution? Given: H₂SO4 (aq) + 2NaOH (aq) → 2H₂O (1) + Na₂SO4 (aq)
15. If 23.0 mL of a 1.00 M Ba(NO3)2 solution was reacted with 55.0 mL of a 0.700 M solution of K3PO4 to produce the solid Ba3(PO4)2 by the balanced chemical equation 3 Ba(NO3)2 (aq) + 2 K3PO4(aq) – Ba3(PO4)2(s) + 6 KNO3(aq) a. What is the limiting reagent? AS b. How many grams of Ba3(PO4)2 will be produced? elomibt.ESE -3HA
9. What is the molarity (M) of a solution if 500 mL of the solution contains 40.85 g of NaHCO₁? 10. If 42.50 mL of a 1.100 M MgCl solution is needed to completely react with 45.0 mL of AgNO, solution, what is the molarity of the AgNO, solution? Hint: use example in Section 9.5 MgCl +2AgNO 2(aq) 3(aq) 2AgCl + Mg(NO3)2(aq) (s) 4
In the following balanced reaction: Pb(NO3)2(aq) + 2KI(aq) → PbI2(s) + 2KNO3(aq) 10.9 g of KI react with a 0.193 mol L-1 solution of Pb(NO3)2. The total solution volume is 0.200L Calculate the number of moles of Pb(NO3)2.
To measure the amount of nickel in some industrial waste fluid, an analytical chemist adds 0.1400M sodium hydroxide NaOH solution to a 23.00g sample of the fluid and collects the solid nickel(II) hydroxide NiOH2 product. When no more NiOH2 is produced, he filters, washes and weighs it, and finds that 0.50g has been produced The balanced chemical equation for the reaction is: Ni2+(aq) + 2NaOH(aq) -> NiOH2(s) + 2Na+(aq) What kind of reaction is this? If you said this was a precipitation reaction, enter the chemical formula of the precipitate. If you said this was an acid-base reaction, enter the chemical formula of the reactant that is acting as the base. If you said this was a redox reaction, enter the chemical symbol of the element that is oxidized. Calculate the mass percent of Ni in the sample. Be sure your answer has the correct number of significant digits.

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