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10 Nov 2019

Write a balanced net ionic equation to explainthe observed pH for each of the solutions tested.


Ammonium Chloride NH4Cl (4.4-4.8pH)
Boric acid H3BO3 (4.4-4.8)
Borax Na2B4O7 (9-10)
Citric acid C6H8O7 (1.8-2.8)
Hydrochloric Acid HCl (1.8-2.8)
Sodium carbonate Na2CO3 (9-10)

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Jamar Ferry
Jamar FerryLv2
30 May 2019

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Related questions

Write (1) a balanced molecular equation, (2) a total ionic equation, and (3) a net ionic equation that would describe a predicted reaction. Please pay attention to details such as charges (e.g. Ba2+ vs. Ba) and states (i.e. (aq), (s), (l), or (g) as appropriate). If a reaction is not predicted to occur (soluble salts on both sides of the equation), only the balanced molecular equation is needed.

 

sodium carbonate + sulfuric acid

Na2CO3 (aq)+ H2SO4(aq) -> Na2SO4(aq) + CO2 (g)+ H2O(l)

Na+(aq)+CO3^2−(aq)+2H+(aq)+SO4^2−(aq) ->H2O(l)+CO2(g)+2Na+(aq)+SO4^2−(aq)

CO3^2−(aq)+2H+(aq) -> H2O(l)+CO2(g)

 

sodiumcarbonate + hydrochloric acid

Na2CO3(aq) + HCl (aq)-> NaCl (aq)+ H2O (l)+ CO2(g)

Na+(aq) + CO3^-2 (aq)

 

potassium chloride + sodium carbonate

KCl (aq)+ Na2CO3 (aq)-> K2CO3 (aq)+ 2NaCl(aq)

 

potassium chloride + silver nitrate

KCl (aq)+ AgNO3 (aq) -> KNO3 (aq)+ AgCl (s)

 

potassium chloride + sodium nitrate

KCl (aq)+ NaNO3 (aq) ->  KNO3 (aq)+ NaCl(aq)

 

nickel chloride + silver nitrate

NiCl2 (aq)+ 2AgNO3(aq) ->  Ni (NO3)2(aq) + 2AgCl (s)

 

nickel chloride + sodium carbonate

KCl (aq)+ Na2CO3(aq) -> K2CO3 (aq)+ 2NaCl(aq)

 

hydrochloric acid + sodium hydroxide

HCl (aq)+ NaOH(aq) ->  NaCl(aq) + H2O(l)

 

Ammonium chloride + sodium hydroxide

NH4Cl(aq) + NaOH(aq) ->  NaCl(aq) + H2O (l)+ NH3(g)

 

sodium acetate + hydrochloric acid

CH3COONa (aq)+HCl (aq) ->  CH3COOH(aq) +NaCl(aq)

 

lead nitrate + sulfuric acid

Pb(NO3)2 (aq)+ H2SO4(aq) -> PbSO4 (aq)+ HNO3(aq)

 

1(a)What is the pH of a buffer system that contains 0.26M hydrocyanic acid (HCN) and 0.30M Sodium cyanide? The Ka of HF is 6.2 x 10-10

1(B)Consider 750mL of the buffer system described above. What are the [HCN] and [CN-] after 0.080 mol of NaOH is added? What is the pH?

1(c)Consider 500mL of the buffer system described above. What are the [HCN] and [CN-] after 0.10 mol of HCl is added? What is the pH?

2.A titration of 15mL of boric acid (H3BO3) required 22mL of 0.25M Ca(OH)2 Write the balanced equation for the reaction of boric acid with Ca(OH)2 and determine how many milligrams of boric acid are present

Part I: pH
Use a pH meter to measure the pH values of 0.10 M solutions of thefollowing
compounds. Also put a drop or two of universal indicator in eachsolution. Record the
pH and the color of each solution.
Sodium chloride, NaCl Sodium hydrogen sulfate, NaHSO4
pH: pH:
Color: Color:
Sodium acetate, CH3COONa Acetic acid, CH3COOH
pH: pH:
Color: Color:
3
Sodium carbonate, Na2CO3 Sodium hydrogen carbonate, NaHCO3
pH: pH:
Color: Color:
For each solution with a pH less than 6 or greater than 8,
write a net ionic equation that accounts for the observed pH.
explain why the color observed with bromcresol green for each ofthe four solutions is resonable given the ph

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