A solution of 118mL of 0.180 M KOH is mixed with a solution of 260mL of 0.190M NiSO4. = 2KOH(aq) + NiSO4(aq) → K2SO4(aq) + Ni(OH)2(s)  What precipitate forms? What is the limiting reactant? How many grams of this precipitate form? W

Q: If 35.8 mL of 0.100 M NaOH is needed to fully react with a 100.0 mL sample of oxalic acid (H2C2O4),…

A: Given data : Molarity of NaOH = 0.100 M Volume = 35.8 mL = 0.0358 L Number of moles of…

Q: Consider the reaction: CaCl:(aq) + 2AgNO3(aq) → Ca(NO3)>(aq) + 2A9CI(s) How many grams of CaCl2…

A: For this question, first find out moles of AgNO3 using molarity formula. Then use mol to mol ratio…

Q: 0.7532 g of copper turnings (molar mass: 63.546 g∙mol–1) are reacted with excess nitric acid.…

A: Disclaimer: In order to obtain copper sulfate the acid used in excess should be sulfuric acid and…

Q: Consider the reaction: CaCl2(aq) + 2A9NO3(aq) → Ca(NO3)2(aq) + 2A9CI(s) How many grams of CaCl,…

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Q: What mass of NaCl is required to precipitate all the silver ions from 30.0 mL of 0.355 M AgNO3…

A: We will use simple mole concept. however, we have to know the following formulas- Molarity=Number of…

Q: what quantity in moles of precipitate will be formed when 268.5 mL of 0.200 M NaBr is reacted with…

A: No. Of moles= molarity×volume Here precipitate is PbBr2 because this is in solid phase ( solid phase…

Q: 100.0 mL of an aqueous solution containing 0.250 M KOH(aq) is mixed with 100.0 mL of an aqueous…

A: First of all, we need to write down the balanced chemical.  The molar mass of Fe(OH)3 = 106.87g/mol

Q: The net ionic equation for the reaction of the strong base Ca(OH)2(aq) with the strong acid HNO3…

A: Net ionic equation is the equation that only shows the elements , compounds that are directly…

Q: Give the complete ionic equation for the reaction (if any) that occurs when aqueous solutions of…

A: Given in the question that, HI and MgSO3 aqueous solutions are mixed .

Q: What mass of precipitate (in g) is formed when 250.0 mL of 0.610 M CuCh is mixed with excess KOH in…

A: Initially, we have: molarity of CuCl2 = 0.610 M Volume of CuCl2 = 250.0 mL Formula to calculate…

Q: 2 The active agent in many hair bleaches is hydrogen peroxide. The amount of H₂O2 in 13.7-g of hair…

A: given, amount of hair bleach = 13.7 g For KMnO4 molarity = 0.174 M volume = 48.9 mL

Q: A 214.0-mL aliquot of 0.360 M  aqueous potassium hydroxide is mixed with 214.0 mL of 0.360 M…

A:

Q: (1) Identify each of the following half-reactions as either an oxidation half-reaction or a…

A: The ionic compound  decomposes to its corresponding ions and give the different product .

Q: 2.) A titration experiment reveals that 11.60 mL of 3.0 M sulfuric acid is required to neutralize…

A: GivenH2SO4(aq.) + 2 NaOH(aq.) → 2H2O(l) + Na2SO4(aq.)Volume of Sulfuric acid = 11.60 mLMolarity of…

Q: What mass of precipitate (in g) is formed when 250.0 mL of 0.200 M CoCl₂ is mixed with excess KOH in…

A: The balanced equation is given as;   CoCl2(aq) + 2 KOH (aq)→Co(OH)2(s)+2KCl(aq) From the question,…

Q: A 57.5 mL sample of a 0.122 M potassium sulfate solution is mixed with 39.0 mL of a 0.126 M lead(II)…

A: Molarity = number of moles of solute/volume of solution (in L)  So, moles = molarity × volume (in…

Q: A 25.0-mL sample of 1.00 M Calcium nitrate solution, Ca(NO3)2, is reacted with 125.0 mL of 0.300 M…

A: Limiting Reagent is the reactant which is completely consumed when a reaction goes to completion.

Q: 5. Calculate the concentration of the hydrochloric acid if a 20.00 mL sample is titrated with…

A:

Q: 150.0 mL of 0.200 M AgNO3 solution is reacted with 100.0 mL of 0.450 M NaBr solution, and the…

A: The balanced reaction taking place is given as, => AgNO3 (aq) + NaBr (aq) -----> AgBr (s) +…

Q: The titration of 25.00 mL of an unknown concentration of H2SO4 solution requires 44.58 mL of 0.42 M…

A:

Q: A titration is performed to determine the amount of sulfuric acid, H2SO4, in a 4.30 mL sample. About…

A:

Q: Calculate the mass (in grams) of PbCl2(s) precipitated by mixing 7.16 mL of a 0.187 M Pb(CH3COO)2…

A: We have to calculate the amount of  PbCl2 precipitation

Q: How many grams of Ag₂CO3 will precipitate when excess K₂CO3 solution is added to 65.0 mL of 0.746 M…

A:

Q: A 55.5mL sample of 0.104M potassium sulfate solution is mixed with 35.5mL of a 0.104M lead(II)…

A: Interpretation: From the given information theoretical yield of PbSO4 in grams is to be determined.…

Q: What minimum mass of iron (II) nitrate must be added to 10.0ml of a 0.0699 M phosphate solution in…

A: The question is based on the concept of Reaction Stoichiometry.   limiting reagent is the reagent…

Q: W

A: In this reaction, NaOH is reacting with FeCl­3 to give NaCl and Fe(OH)3 is getting precipitated. In…

Q: If 355 mL of 0.325 M Pb(NO₃)₂ is added to 315 mL of 0.225 M K₃PO₄, how many moles of Pb₃(PO₄)₂…

A:

Q: if 30.0 g of NaOH is added to  0.800L of 1.00M Zn(NO3)2, what is the mass in grams of Zn(OH)2 will…

A: The balanced equation for the given precipitation reaction is as follows.…

Q: Solution A is 0.2400 M Ca(NO3)2(aq). Solution A is diluted by a factor of 3 to form Solution B.…

A: The reaction taking place is  3As2O3 + 4NO3- + 7H2O + 4H+ → 6H3AsO4 + 4NO Balancing explanation :…

Q: how many grams of precipitate will be produced

A:

Q: How many grams of Cu(OH)2 will precipitate when excess NaOH solution is added to 72.0 mL of 0.578 M…

A:

Q: Lead(II) nitrate and ammonium iodide react to form lead(II) 10dide and ammonium nitrate according to…

A:

Q: W Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of Na2CO3…

A: The question is based on the concept of chemical reactions. we need to write net Ionic equation for…

Q: Fe(II) can be precipitated from a slightly basic aqueous solution by bubbling oxygen through the…

A: The number of moles of Fe(II) is calculated as, 4Fe(OH)++4OH-(aq)+O2(g)+2H2O(l)→4Fe(OH)3(s) Moles of…

Q: Suppose 65.2 mL of a 0.155 M solution of Na₂SO4 reacts with 153 mL of a 0.279 M solution of MgCl₂ to…

A:

Q: A chemist performs a gravimetric analysis. The chemist combines 1.00 L of 2.00 M AGNO, (ag) with…

A: Given: Concentration of AgNO3 = 2M Concentration of NaCl = 4M Volume of AgNO3 = 1 L Volume of NaCl =…

Q: Consider the following reaction H2S (g) + FeS(s) + CO2(g) →FeS2(s) + HCO2H(aq) If 2.00 g of each…

A: Molar mass of H2S =34g/mol Molar mass of FeS =88 g/mol Molar mass of CO2 =44g/mol  Given mass of…

Q: 8) What is the molarity of the solution containing 234 g NaCl in 3.00 L of solution?

A: Solving only first question in accordance with guidelines.

Q: 1. Determine the mass in grams of Lead(II) lodide th

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: How many grams of Cu(OH)2 will precipitate when excess KOH solution is added to 41.0 mL of 0.618 M…

A: To solve this problem we will use the given balanced chemical equation.

Q: How many grams of Ag₂CO3 will precipitate when excess Na2CO3 solution is added to 49.0 mL of 0.590 M…

A:

Q: How many grams of Cu(OH)2 will precipitate when excess KOH solution is added to 69.0 mL of 0.584 M…

A: The number of moles of substance is defined as the ratio of given mass to that of molar mass.  The…

Q: A 57.0 mL sample of a 0.118 M potassium sulfate solution is mixed with 38.0 mL of a 0.122 M…

A: The balanced reaction taking place is given as, => K2SO4 (aq) + Pb(C2H3O2)2 (aq) → 2 KC2H3O2 (aq)…

Q: 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…

A: The objective of this question is to determine the number of moles of Mg3(PO4)2 that will…

Q: CaCl2(aq) is reacted with 125.0 mL of 0.17M  solution of Na3PO4(aq) Given the reaction : 2Na3PO4(aq)…

A:

Q: Calculate the number of milliliters of 0.793 M NaOH required to precipitate all of the Fe³+ ions in…

A: Molarity is defined as the ratio of the number of moles of the substance to that of the volume of…

Q: 100. mL of 0.10 M CaCl, is mixed with 50.0 mL of a 0.10 M solution of either Al₂(SO4)3, Na₂SO4, or…

A: A question based on mole concept. 3 probable chemical equations are given and the most appropriate…