Q: → PBSO4 + MnOq d PbO, + Mn²+ + SO,²- - e HNO, + Cr,O,²- → Cr* + NO;
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Q: A mixture of 2.00 g BaCl2.2H2O (molar mass = 244.2g/mol) and 1.00 g of NazPO4.12H20 (molar mass =…
A: Given that: Mass of BaCl2.2H2O = 2.00g Molar mass of BaCl2.2H2O = 244.2g/mol Moles =…
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Q: What is the percentage of metal in the compound Iron (III) Chromate (Fe2(CrO4)3)? ОА. 24.30% о в.…
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Q: If 2.73 g KHC2O4·H2C2O (three ionizable protons) having 2.0% inert impurities and 1.68 g KHC8H4O44…
A: Given: 2.73 g KHC2O4·H2C2O (three ionizable protons) having 2.0% inert impurities 1.68 g KHC8H4O4…
Q: Is there a reaction between: F- and Na + F2 and Na + Cl2 and Fe2 + I2 and Br- Cl2 and I-
A: Is there a reaction between F- and Na + F2 and Na + Cl2 and Fe2 + I2 and Br- Cl2 have to be given,
Q: 9. Give the net ionic equation for the following: N22SO4(aq) + Ga(NO3)3(aq) - → ee
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Q: hydroxide ions plus iron (II) ions * FeH2O FeOH FeO 2Fe(OH)2
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Q: I. i. Pt|Cra), Cr,0ag)||CLO3(aq), Cliag)|Pt j. Mn(s)|Mnaq)||Htaq)\H2c9) \Pt
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Q: Write the name and oxidation state of pt
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Q: Complete and balance the following equations. If no reac-tion occurs, write NR:(a) H₃PO4(l)+ NaI(s)…
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Q: Give an example of ionisation isomerism.
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Q: 1) chlorides formed by chromium( can be more than one answer) a) Cr3Cl b) CrCl3 c) CrCl 2 d) CrCl4…
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Q: What is the equation for the reaction of Mg(s) with CuSO4(aq)?
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Q: What is the percentage of metal in the compound Iron (III) Chromate (Fe2(C О А. 24.30% о в. 58.23% О…
A: Calculate percentage as below
Q: A mixture of 0.560 g BaCl, 2H2O (molar mass = 244.2g/mol) and 1.44 g of NazPO4 12H20 (molar mass =…
A: 2Na3PO4 + 3BaCl2-----> Ba3(PO4)2 (s) + 6NaCl Mass of BaCl2.2H2O = 0.560 g Molar mass of…
Q: Iron(III) chloride is used to test the purity of your aspirin. Why does salicylic acid reacts with…
A: Given: Iron (III) i.e. Fe3+ reacts with salicylic acid.
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Q: What is the milliequivalents of 0.980 g of Na2CO3 (MW=105.99)?
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Q: H*(ag) + Cr,O,² (aq) + C,H;OH(1) acid Cr*(aq) + CO2(g) + H;O(1)
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- (a) Given that Kb for ammonia is 1.8 x10-5 and that forhydroxylamine is 1.1 x 10-8, which is the stronger base?(b) Which is the stronger acid, the ammonium ion or thehydroxylammonium ion? (c) Calculate Ka values for NH4+and H3NOH+.5. Which of the following equations shows that isoquinoline, C9H;N, behaves as a Bronsted-Lowry base in water? a) CóH;N(aq) + H2O(1) = b) CH;N(aq) + H2O(1) c) C9H;N(aq) + OH¯(aq) = d) CoH;N(aq) + H;O*(aq) e) CoH;NH*(aq) + H2O(!) C9H;NH*(aq) + OH (aq) = C9H&N°(aq) + H;O*(aq) C9HN¯(aq) + H;O(!) = C9H;NH*(aq) + H2O(1) = C9H;N(aq) + H;O*(aq)Propose two molecular formulas for each of the following molecular ions: (a) 72; (b) 100; (c) 73.
- The following questions concern the reaction HA(aq) + B(aq) ⇄ HB1+(aq) + A1–(aq). What can you say about: (a) the magnitude of K for this reaction (K >> 1 or K << 1 or K ≈ 1), (b) the relative concentrations of HA and HB1+ ([HA] >> [HB1+] or [HA] << [HB1+]), and (c) the pH of the solution that results from reacting equal mole quantities of HA with B, when HA is a weaker acid than HB1+. K_____ Relative Concentration_____ pH_____HA is a weak acid and B is a strong base. K_____ Relative Concentration_____ pH_____ HA is a strong acid and B is a strong base. K_____ Relative Concentration_____ pH_____ HA is a strong acid and B is a weak base. K_____ Relative Concentration_____ pH_____Given the Ka values (in parentheses) for the following acids: HSO4– (Ka= 1.2 x 10–2); HNO2 (Ka= 4.0 x 10–4); HC2H3O2 (Ka= 1.8 x 10–5); Calculate Kc values for the following acid-base equilibria: (a) HSO4–(aq) + C2H3O2–(aq) ⇌ HC2H3O2(aq) + SO42–(aq) (b) HC2H3O2(aq) + NO2–(aq) ⇌ HNO2(aq)+ C2H3O2–(aq)(a) Given that Ka for acetic acid is 1.8 x 10-5 and that forhypochlorous acid is 3.0 x 10-8, which is the stronger acid?(b) Which is the stronger base, the acetate ion or the hypochloriteion? (c) Calculate Kb values for CH3COO- and ClO-.
- The acid HA has pKa 7.00. (a) Which is the principal species, HA or A, at pH 6.00? (b) Which is the principal species at pH 8.00? (c) What is the quotient [A]/[HA] at (i) pH 7.00; (ii) at pH 6.00?(2) Caffeine (C8H10N4O2) is a weak base with a pKь of 10.4. Calculate the pH of a solution containing a caffeine concentration of 455 mg/L.(b) Calculate the pH of 0.0005 mol dm-3 ethanois acid when its pKa = 4.75 CH;COOH() -> CH;COO (a H(a + Ka = pH =
- In the following reaction in aqueous solution, the base reactant is and its conjugate acid product is CH3COOH(aq) + NH3(aq) CH3COO (ag) + NH4 (ag) O NH3: NH4 NH3: CH3COO CH3COOH; NH4 CH3COOH; H30+ CH3COOH; CH3CO*Dicarboxylic acids have two dissociation constants, one for the initial dissociation into a monoanion and one for the second dissociation into a dianion. For oxalic acid, HO2C—CO2H, the first ionization constant is pKal = 1.2 and the second ionization constant is pKa2 = 4.2. Why is the second carboxyl group far less acidic than the first?Calculate the Ka's for the following acids: (a) Citric acid, pKa = 3.14 (b) Tartaric acid, pKa = 2.98