I need answers for the questions. Questions 1. Write balanced molecular and ionic equations for each…
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Question “I need answers for the questions. Questions 1. Write balanced molecular and ionic equations for each…”
need answers for the questions.
Questions 1. Write balanced molecular and ionic equations for each successful precipitation reaction that you observed. a. b. Were the solubility rules completely adequate? Explain. 2. Describe how red litmus paper is affected by acids and bases. a. b. Describe how blue litmus paper is affected by acids and bases. Which litmus paper would you use to test for an acid? Why? c. d. Which litmus paper would you use to test for a base? Why? Write balanced molecular and ionic equations for each reaction of a solid with HCl. 3. a. Write balanced molecular and ionic equations for each neutralization b. reaction in which heat was evolved.
. Results 1. Testing the solubility rules 1gtcoti3 b sscisds NaBr Na SO NaOH Solurde No Heat No reaction Do hat Mscluble Nohat Na,CO, Solubla No het Na Yation No feaden Solubeo No heat Scubla NH NO Selulole o heat Solble Seluble Cder dhomes ho Ba(NOs)2 | Arecipitte teodhte peaph SoctePeptate sobble no eat Seluble no readken white Calor dhanc Chanze no hedt no faschon cordy soluble no heast AgNO, nsole No heut Precipbte WD veachion duale No renctesn te wte cole Pb(NOs)2 Caor chonge Precipitate cavdy Seluble Ni(NOs)2 Preciptere no heat C+ alers 33
eoiblo os PIYO Precipitote disappented 2. Looking at dacids and bases HCI+ precipitate From Ni (NO2)s + NaOH gas ewles HCI+CaCO, afu Blue Litmus Paper Red Litmus Paper le idolo Color changed to Pink No reaction HС Color changed to pnk Do veaction HС-Но, No reuction No veachn NHS vityo coler changed Onid to dark blue Color changal NaOH Heat Evolved? No heat HCI NH evolues eligt НС-Н,02 + NaОН
Answer
1a) Molecular equation: Na2SO4 (aq), Ba(NO3)2 [aq] – BaSO4 s) + 2NaNO3 aq
Ionic equation: Ba 2+ +SO 4 4- – BASO4 (s).
Molecular equation: Ba (NO3) (aq), + 2NaOH[aq] – Ba(OH] _(s)+ 2NaNO3[aq]
Ionic equation: Ba + (aq), + 2OH (aq), – _(aq), – Ba(OH). 2_(s)
Molecular equation: Ba(NO3)2 (aq), + Na2CO3 (aq), –> BaCO3(3)(s) + 2NaNO3(3)(aq),
Ionic equation: Ba 2+ (aq) + Co3 2 – _(aq), – BaCO3(3)(s)
Molecular equation: 2AgNO3(aq), + Na2SO4 (aq). – Ag2SO4[s] + 2NaNO3(aq).
Ionic equation: 2Ag + (aq) + SO 4- (aq) – AgSO (4 )
Molecular equation: AgNO3 (aq), + NaOH (aq),- AgOH(s), + NaNO3 (+aq).
Ag+(aq) + OH–(aq) – AgOH(s)
Molecular equation: 2AgNO3 (aq), + Na2CO3 (aq), – Ag2CO3 (3(s)) + 2NaNO3 (4(aq),
2Ag+ + CO32- – Ag2CO3(s)
Molecular equation: Na SO (aq), + Pb(NO3)2 (aq), – 2NaNO (aq), + PbSO (4 ) (s)
Pb2+ (aq) + SO42-(aq) – PbSO4(s)
Molecular equation: Pb(NO3)2 (aq), + 2NaOH [aq] – 2NaNO (aq), + Pb (OH)2 (s)
Pb2+ (aq) + 2OH–(aq) – Pb(OH)2(s)
Molecular equation: Na2CO3 [aq] + Pb(NO3)2[aq] – 2NaNO (aq] + PbCO3[s)
Pb2+ (aq) + CO32-(aq) – PbCO3(s)
Molecular equation: Na2SO4 (aq), Ni(NO3)2 (aq), – NiSO4 (+ 2NaNO3+(aq).
Ni+2(aq) + SO4-2(aq) – NiSO4 (s)
Molecular equation: Ni(NO3)2 (aq), + 2 NaOH[aq] – NiOH)2(s), + 2 NaNO3[aq]
Ni+2(aq) + 2HO–(aq) – Ni(OH)2 (s)
Molecular equation: Na2CO3 + Ni(NO3)2 – NiCO3 – 2NaNO3 – aq
Ni+2(aq) + CO3-2(aq) – NiCO3 (s)
1b) Soluble compounds with group 1A ions and nitrates or sulphates Hydroxide ions can be soluble in group 1A ions, ammonium, Sr2+ and Ba2+. Ammonium ion and group 1A ions are also compatible with carbonates and phosphates.
2a. Red litmus paper becomes blue when it comes into contact with base, while it remains red when in contact with acid or neutral solutions. The presence of weak diprotic acids in red litmus papers causes hydrogen ion to react with the base solution to form conjugate bases.
2b. Blue litmus paper becomes red when it comes into contact with acid, whereas it stays blue when treated with neutral solution and base. Blue litmus paper’s pigment reacts with hydrogenions, which tunes the bond to produce a longer wavelength. Red color
2c) Acid blue litmus paper is used to measure pH change below 4.5.
2d) Base red litmus paper is used to represent the color change of pH above 8.3. It turns blue when it reaches that level.
3a) CaCO3(s) + 2HCl(aq) – CaCl2(aq) + CO2(g) + H2O(l)
Ionic equation: CaCO3 (s) + 2H+ (aq), – Ca2+ (+aq), + CO2(g), + H2O[l]
3b) In both reaction heat is not developed HCl + NaOH + H2H3O2 and HCl+ NH3
Conclusion
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