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- Balance the following net ionic equation (there is one mole of (NH4)3PO4●12MoO3 in the balanced equation- do NOT change this coefficient): HPO42-(aq) + NH4+(aq) + MoO42-(aq) + H+(aq)(NH4)3PO4●12MoO3(s) + H2O (l)Balance the following equation. ___ M2CO3 (s) + ____ HCI(aq) --->___ CO2 (g) + ____ MCI (aq) +____ H2O(I) With the chemical equation above the following data was obtained: Mass of unknown + weighing boat - 2.87g Mass of weighing boat - 2.14g Volume of 1.0 M HCI used 19.11 mL What is the # of moles of HCI # of moles of unknown carbonate used The molar mass of unknown carbonate What is the identity of the unknown carbonate?The following reaction occurs in basic solution: _ H2O(aq) + _ MnO4–(aq) + _ ClO–(aq) → _ MnO2(s) + _ ClO4–(aq) + _ OH–(aq) When the equation is properly balanced, what is the sum of the lowest whole-number coefficients? a. 9 b. 10 c. 20 d. 12 e. 6
- when the following equation is balance, the coefficient of H2 is K(s)+H2O(L)-->KOH(aq)+H2(g) answers options (a)1 (b)2 (c)3 (d)4 (e)5Aqueous sodium hypochlorite (NaOCl, household bleach) is a strong oxidizing agent that reacts with chromite ion [Cr(OH)4-] in basic aqueous solution to yield chromate ion CrO42- and chloride ion Cl-. The next ionic equation is: ClO- (aq) + Cr(OH)4-(aq) ------> CrO42-(aq) + Cl-(aq) Unbalanced Balance the equation using the method described in section 1 of the Electrochemistry chapter.Can I please get assistant with the following problem? Write a balanced complete ionic equation for the following ionic solid. Assume A is a metal ion and B is an anion. For example, CaCO3(s) ⇌ Ca2+(aq) + CO32-(aq) A2B2(s) ⇌ x A+(aq) + y B-(aq) What is the value of y?
- Identify the spectator ions in the following balanced molecular equation: KBr (aq) + AgNO3 (aq) → AgBr (s) + KNO3 (aq) Group of answer choicesThe Original volume of unknown NaCl solution = 98.407mL The concentration of Ag + within the 10 mL unknown NaCl solution after AgCl is added [Ag+] = 4.71370e^-10 Calculate Calculate the mass of NaCl in the 10 mL unknown solution. Show your work.? Hint: mole = molarity x L; mass = mole x molar mass AgCl(s)⇌Ag+(aq)+Cl−(aq) Ksp=[Ag+][Cl−]KHP (aq)+NaOH (aq)-->NaKHP (aq)+H2O(l) Trial Vi (mL) Vf (mL) 1 36.19 48.56 2 3 A student masses out 1.096 grams of KHP, which is dissolved in 25.00 mL of DI water. This KHP solution is titrated with NaOH, as shown in the equation above. Calculate the molarity of the NaOH solution.