Which metal dissolves in sulfuric acid to produce an aqueous solution and no precipitate? a. lead...
Question:
Which metal dissolves in sulfuric acid to produce an aqueous solution and no precipitate?
a. lead
b. chromium
c. barium
d. silver
Sulfuric acid:
Sulfuric acid dissociates completely in water and hence it is a strong acid. It is composed of elements like sulphur, oxygen, and hydrogen. It is corrosive in nature and is dangerous acid. It can be used to dissolve certain metals in solution.
Answer and Explanation: 1
Become a Study.com member to unlock this answer! Create your account
View this answerThe answer is b. chromium.
No precipitate will form when chromium is dissolved by sulfuric acid since the sulfate salt of chromium is soluble in...
See full answer below.
Ask a question
Our experts can answer your tough homework and study questions.
Ask a question Ask a questionSearch Answers
Learn more about this topic:
Get access to this video and our entire Q&A library
What is Acid in Chemistry? - Definition & Overview
from
Chapter 16 / Lesson 22
80K
Explore acids in chemistry. Learn the definition of an acid and understand its different types. Discover various examples of acids and see their characteristics.
Related to this Question
- Of the metals below, which of the following will not dissolve in an aqueous solution containing nickel ions? A) Aluminum B) Chromium C) Barium D) Tin E) Potassium
- (a) Does a precipitate form when sulfuric acid is added to lead nitrate? (b) If so, what is the reaction? (c) Why does the precipitate form?
- Which of the following insoluble metal hydroxides will dissolve in an excess of aqueous ammonia? (a) Zn(OH)2 (b) Cr(OH)3 (c) Fe(OH)2 (d) Ni(OH)2 (e) Cd(OH)2
- Which of the following metals will dissolve in nitric acid but not hydrochloric? A) Fe B) Pb C) Cu D) Sn E) Ni
- Which of the following substances is more soluble in a perchloric acid solution then in a barium hydroxide solution? A) AgCl B) Pb(OH)_2 C) CaF_2 D) HI E) Fe_3(PO_4)_2
- What precipitate is likely to form when aqueous solutions of sulfuric acid (H2SO4) and barium chloride (BaCl2) are mixed, according to the general solubility rules? If it is unlikely that a precipitate will form, indicate which solubility rules are applic
- Which metal will not react with copper(II) chloride in solution? a. Silver b. Iron c. Lead d. Zinc
- Which of the following metals dissolves in HNO_3 but not in HCl? a) Fe b) Au c) Ag
- Which of the following metals will dissolve in nitric acid but not hydrochloric acid? a. Cd b. Cr c. Mn d. Ag e. Al
- Which of the hydrogen halides react(s) with AgNO3(aq) to given a precipitate that dissolves in Na2S2O3(aq)?
- Which of the following should react with sulfuric acid to form an insoluble solid (a precipitate)? a. KCl b. Na3PO4 c. Mg(NO3)2 d. Ca(NO3)2 e. none of the above
- Which is more likely to dissolve in an acidic solution, silver sulfide or silver chloride?
- Which of the following substances is more soluble in a perchloric acid solution then in a barium hydroxide solution? a. AgCI b. Pb(OH)_2 c. CaF_2 d. HI e. Fe_3(PO_4)_2
- Given the following equation for a precipitation reaction, which species is the precipitate? 2 AgNO_3(aq) + Na_2S(aq) to 2 NaNO_3(aq) + Ag_2S(s) A. AgNO_3. B. Na_2S. C. NaNO_3. D. Ag_2S.
- Which of the following insoluble metal hydroxides will dissolve in an excess of aqueous ammonia?
- What precipitate forms when aqueous lead (II) nitrate reacts with aqueous sodium sulfate?
- What ions does chromium (III) iodide, CrI3, produce in an aqueous solution?
- Suppose 500 mL of a 0.0035 M solution of lead nitrate is reacted with sulfuric acid. What mass of lead sulfate should precipitate?
- Mn, Cu, Au, Ag, Ni. (a) Which metals would dissolve in HCl? (b) Which metals would dissolve in HNO_3?
- Which of the following will show a precipitate with the addition of 2.0 M sulfuric acid? a. KBr b. NaNO3 c. NiBr2 d. LiCl e. K2CO3 f. KHCO3 g. BaCl2
- Which of the following compounds to precipitate Mg^{2+} from the aqueous solution of MgCl2? what's the equation for the reaction. a. Na2S b. Na2CO3 c. NaI d. NaNO3
- What ions does barium chloride, BaCl2, produce in an aqueous solution?
- Which of the following will be more soluble in an acidic solution than in pure water? a.AIPO_4 b.CsCIO_4 c.AgCl d.Sn(OH)_2 e.BaSO_4
- (a) What is a net ionic equation for the reaction between barium nitrate and potassium sulfate? (b) Determine whether or not this reaction will lead to a precipitate.
- Which combination will produce a precipitate? a. AgNO_3(aq) and Ca(C_2H_3O_2)(aq) b. NaOH(aq) and Fe(NO_3)_3(aq) c. NH_4OH(aq) and HCl(aq) d. NaCl(aq) and HC_2H_3O_2(aq) e. NaOH(aq) and HCl(aq)
- Which combination will produce a precipitate? a. NaCl(aq) and HC2H3O2(aq) b. NaOH(aq) and Fe(NO3)3 (aq) c. NH4OH(aq) and HCL(aq) d. KNO3(aq) and AlCl3(aq) e. Ca(C2H3O2)2(aq) and AgNO3(aq)
- Which of the following compounds will be more soluble in acidic solution than in neutral solution? a. BaCO_3. b. CuS. c. AgCl. d. Pbl_2.
- What is the structure of the precipitate that forms after sulfuric acid has been added to the mixture of p-aminobenzoic acid in ethanol? Why do you need to add more acid even after the precipitate starts forming? Explain why benzocaine precipitates during
- If after precipitation of the Group I cations as chlorides by the reaction with HCl nearly all of the precipitate dissolves in hot water. What ion is most probably present and which ions are most probably absent?
- If after precipitation of the Group I cations as chlorides by the reaction with HCl, nearly all of the precipitate dissolves in the hot water, what ion is most probably present and which ions are most
- Which combination of dilute aqueous reagents will not produce a precipitate? and why will it not form (A) AgNO3 + HCl (B) NaOH + HClO4 (C) BaBr2 + Na2SO4 (D) ZnI2 + KOH
- (a) What is the precipitate which forms and then redissolves upon adding H 2 S O 4 to the mixture of K + , [ A l ( H 2 O 2 ) 2 ( O H ) 4 ] , and O H ? (b) Calculate the volume of 6.0 M sulfuric acid, H 2 S O 4 , solution required to neutralize the
- What is the precipitate of K_2CrO_4 + Al_2(SO_4)_3 \to?
- A solution of K2O is mixed with a solution of FeBr2. A black precipitate is formed. What is the net ionic equation for the reaction? What is the black precipitate?
- Which will precipitate first when AgNO3 is added to a solution containing equal concentrations of Br-, Cl-, and I- ions? A. AgBr B. AgCl C. AgI D. AgNO3 E. No precipitate will form.
- Which of the following will be more soluble in an acidic solution than in pure water? a. CaSO4 b. AlPO4 c. AgCl d. Sn(OH)2 e. KCIO4
- Which of the following mixtures of reactants will NOT form a precipitate? a. Zn(NO_3)_2 and Na_2S (aq) b. Rb_2S (aq) and LiCl (aq) c. K_2CO_3 (aq) and Mg(NO_3)_2 (aq) d. Na_3PO_4 (aq) and AgNO_3 (aq)
- When aqueous solutions of iron (III) sulfate, (Fe_2(SO_4)_3) and sodium hydroxide were mixed, a precipitate is formed. What is the precipitate?
- Which of the following will be more soluble in an acidic solution than in pure water? a.BaSO_4 b.AgCl c.RbClO_4 d.CaCO_3 e.Zn(OH)_2
- What is the precipitate that forms when an aqueous solution of FeCl_3 reacts with an aqueous solution of (NH_4)_2CO_3? (a) FeCO_3 (b) NH_4Cl (c) Fe_3(CO_3)_2 (d) Fe_2(CO_3)_3.
- Which one of the following combinations would NOT form a precipitate in aqueous solution? A) Sr(NO_3)_2 and NaOH. B) AgNO_3 and KBr. C) Zn(C_2H_3O_2)_2 and Na_2S. D) Pb(NO_3)_2 and Na_2SO_4. E) All of the combinations will form precipitates.
- Which of the following aqueous solutions will react with solid aluminum metal? a. AgNO3 b. Na2CO3 c. CuSO4 d. CaCl2 e. Pb(NO3)2
- Which of these compounds are soluble in water? - KCl - H2SO4 - BaSO4 - Ca(OH)2 - AgNO3 - NaCl - Al(OH)3 - AgCl
- 1 liter of a 1 M lithium hydroxide solution is added to 1 liter of a 1 M barium chloride solution, and a precipitate forms. What ions are left in solution after the reaction is complete?
- An excess of aqueous AgNO_3 reacts with 24.5 ml of 5 M K_2CrO_4 (aq) to form a precipitate. What mass of the precipitate is formed?
- For which pair of the cations would the addition of dilute hydrobromic acid precipitate one, but not the other? A) Ag^+ and Ca^{2+} B) Hg_2^2 C) Ba_2 and Na^+ D) Ca^{2+} and Ba^{2+} E) Pb_2 and Ag^+
- What ions are present in an aqueous solution of silver nitrate, AgNO3(aq)?
- When silver nitrate (AgNo3) and barium chloride (BaCl2) are mixed, a white solid precipitate is formed. What is the identity of the precipitate?
- A beaker contains a solution that is 0.50M in Au^{3+} ion and 0.25 M in Ag^+ ion. A solution of sodium chloride is slowly dripped into the beaker with stirring. Which ion will precipitate first, the gold or the silver? Explain. K_{sp, AuCl_3} = 3.2\times1
- What is the mass of the precipitate formed when 45.0 milliliters of 0.250 M barium chloride solution reacts with 2.00 grams of copper (II) sulfate pentahydrate?
- If a 0.100 molar solution of NaOH is added to a solution containing0.200 molar Ni^{2+}, 0.200 molar Ce^{3+}, and 0.200 molar Cu^{2+}, which metal hydroxide will precipitate first? K_{sp} (Ni(OH)_2) = 6.0 times 10^{-16}, K_{sp} (Ce(OH)_3) = 6.0 times 10^{-
- What is the formula of the precipitate (if any) that is formed in the reaction between Ba(NO3)2(aq) and MgSO4(aq)?
- (a) What is a net ionic equation for the reaction between sodium fluoride and magnesium iodide? (b) Determine whether or not this reaction will lead to a precipitate.
- Which of the following reagents would you add to a solution of chromium(III) chloride to precipitate chromium(III) hydroxide? a. Na_2S. b. Fe(OH)_2. c. ZnS. d. AlPO_4. e. NaOH. f. CaCO_3. g. Na_3PO_4. h. K_2CO_3.
- What is the formula of the precipitate formed when a solution of NaOH is mixed with a solution of FeCl3?
- Which of the following solutions could be mixed together to form a precipitate of silver sulfide? A. AgNO_3 and Na_2S. B. AgNO_3 and Na_2SO_4. C. AgClO_4 and CS_2. D. None of the above solutions, when mixed, yield a precipitate of silver sulfide.
- An excess of aqueous AgNO_3 reacts with 20 mL of 5 M K_2CrO_4 (aq) to form a precipitate. What mass of precipitate is formed?
- An excess of aqueous AgNO3 reacts with 41 mL of 5 M K2CrO4(aq) to form a precipitate. What is the precipitate?
- What is the formula of the precipitate formed from the precipitation reaction of Pb(NO_3)_2 and NaI?
- What precipitate (if any) will form if the following solutions are mixed together? Hg2(NO3)2(aq) + CuSO4(aq)
- Does a precipitate form when aqueous solutions of hydrochloric acid and sodium sulfide are mixed? If so, write the formula of the precipitate.
- Silver metal may be precipitated from a solution of silver nitrate by placing a copper strip into the solution. What mass of AgNO3 would you dissolve in water in order to get 1.00 g of silver?
- Which of the following salts would not form a precipitate in an aqueous solution? a. Cu(NO3)2 b. Cu(OH)2 c. CaCl2 d. Pb3(PO4)2
- What anions form a pale yellow precipitate with AgNO3(aq) in an acidic solution?
- What is the structure of the precipitate that forms after sulfuric acid has been added to the mixture of p-aminobenzoic acid in ethanol? Why do you need to add more acid even after the precipitate sta
- Which combination will produce a precipitate? a. silver nitrate and calcium acetate b. sodium hydroxide and ferric nitrate c. ammonium hydroxide and hydrochloric acid d. sodium chloride and acetic acid e. sodium hydroxide and hydrochloric acid
- Identify any precipitates that form from the mixture of aqueous solutions of 1.0 M sulfuric acid and 1.0 M NaOH.
- Which is/are not soluble in water? (I) NaOH \\(II) BaCO_3 \\(III) AgCl \\(IV) (NH_4)_3PO_4 \\(V) FeCl_2 1. (I) only 2. (III) only 3. (V) only 4. (II) and (III) 5. (II) and (V)
- Which combination will produce a precipitate? a) AgNO3 (aq) and Ca(C2H3O2) (aq) b) NaOH (aq) and Fe(NO3)3 (aq) c) NH4OH (aq) and HCl (aq) d) NaCl (aq) and HC2H3O2 (aq) e) NaOH (aq) and HCl (aq)
- What kind of precipitate does BaCl + Na_2S form?
- Which of the following will occur when solutions of CuSO4(aq) and BaCl2(aq) are mixed? a. a precipitate of CuCl2 will form; Ba2+ and SO42- are spectator ions b. a precipitate of CuSO4 will form; Ba2+ and Cl- are spectator ions c. a precipitate of BaSO4 wi
- Which of the following metals will NOT dissolve in a solution containing 1 mol / L H + ? Select one or more: (a) Cu (b) Mn (c) Au (d) Zn (e)Mg (f) Ag
- (a) Does a precipitate form when sodium oxalate is added to lead nitrate? (b) If so, what is the reaction? (c) Why does the precipitate form?
- Combining aqueous solutions of BaI2 and Na2SO4 affords a precipitate of BaSO4. Which ion(s) is/are the spectator ions in the reaction?
- 1.) When aqueous solutions of lead(II) nitrate and potassium iodide are mixed, what is the formula for the insoluble solid (precipitate) that forms? a.) KNO_3(s) b.) PbI(s) c.) PbI_2 d.) Pb(NO_3)_2(s)...
- If 24.0 mL of 0.170 M sodium iodide reacts with a 0.209 M mercury (II) nitrate solution to form HgI2 precipitate, what is the mass of HgI2 formed?
- Which of the following compounds will be more soluble in acidic solution than in neutral solution? 1. BaCO_3 2. CuS 3. AgCl 4. PbI_2
- Which salt would you expect to dissolve more readily in acidic solution, barium sulfate or barium fluoride? Explain.
- Lead (II) iodide is a bright yellow solid that does not dissolve in water. What two solutions can be mixed that would result in a precipitate of lead (II) iodide formed?
- Which of the following will be more soluble in an acidic solution than in pure water? a) BaSO_{3} b) Be(OH)_{2} c) RbClO_{4} d) Ag_2SO_{4} e) AgCl
- Which anions are absent in a solution that forms a precipitate upon the addition of BaCl2(aq)?
- A barium mineral was dissolved in hydrochloric acid to give a solution of barium ion. An excess of potassium sulfate was added to 50.0 mL of the solution, and 1.128 g of barium sulfate precipitate formed. Assume that the original solution was barium chlor
- Which of the following mixtures of aqueous solutions would form precipitates? a. NaOH and FeCl_3. b. Pb(NO_3)_2 and CaCl_2. c. AgNO_3 and NaCH_3CO_2. d. NaCl and Hg(NO_3)_2.
- Which of the following ionic compounds will form a precipitate in water? a. PbCO_3. b. Na_2CO_3. c. Pb(NO_3)_2. d. Na_2NO_3.
- Does a precipitate form when aqueous solutions of barium chloride and sodium sulfate are mixed? If so, write the formula of the precipitate.
- A solution is 5.0 x 10^-5 M in each of these ions: Ag^+, SO_4^2-, Cl^-, CO3^2 Which precipitate will form? Ag_2SO_4 (K_sp= 1.12 x 10^-5) AgCl (K_sp = 1.77 x 10^-10) Ag_2CO_3 (K_sp= 8.46 x 10^-12)
- A solution of Li_2S is mixed with a solution of FeCl_2. A black precipitate is formed. State the net ionic equation for the reaction, and identify the black precipitate.
- Aqueous solutions of cesium chlorate and iron(II) nitrate are poured together and allowed to react. What is the identity of the precipitate, if one is produced? a) Fe(NO3)2 b) This reaction does not
- A salt was completely soluble in water. When this solution was treated with AgNO_3 no precipitate was formed. What anions could be present?
- What solid is formed upon addition of silver nitrate to a solution of cobalt chloride?
- Which of the following compounds is/are soluble in water? I) zinc acetate (Zn(CH_3CO_2)_2). II) barium sulfate (BaSO_4). III) iron(III) hydroxide (Fe(OH)_3).
- What if any precipitate will form from the mixing of these pairs of solutions? A) MgCl2 and AgNO3 B) KCl and (NH4)2SO4
- What chemical is used to dissolve copper(II) oxide and make a solution of copper(II) ions? Options: \\ A. acetic acid B. hydrochloric acid C. sulfuric acid D. nitric acid E. phosphoric acid
- Which of the following will be more soluble in an acidic solution than in pure water? AgCl Sn(OH)_2 CaSO_4 KCIO_4 KCIO_4 CaCO_3
- When solutions of barium hydroxide and sulfuric acid are mixed, the net ionic equation is Ba^(2+)(aq) + SO_4^(2-)(aq) \to BaSO_4(s) because only the species involved in making the precipitate are included. State whether the above statement is true or fal
- A solution contains 1.04 x 10-2 M silver acetate and 1.21 x 10-2 M barium nitrate. Solid ammonium sulfate is added slowly to this mixture. a. What is the formula of the substance that precipitates first? b. What is the concentration of sulfate ion when th
- Identify a reagent or reagents that would do the following: a) precipitate mercury (I) ions but not nickel (II) ions b) precipitate copper (II) ions but not iron (III) ions c) precipitate cobalt (II) ions but not aluminum ions
- Predict which of the following combinations of compounds would produce a precipitate. State what the precipitate will be if there will be one. a) barium hydroxide and ammonium phosphate b) silver nitrate and potassium acetate c) copper(I) sulfate and sodi
- Which of the following substances are not ionized in an aqueous solution? Explain. a) HI \\b) KBr \\c) H_2SO_4 \\d) HNO_2 \\e) AgCl \\f) Ca(NO_3)_2
- You were given an unknown which gave precipitates with all four test solutions, 1 M H2SO4 0.25 M (NH4)2C2O4 1M K2CrO4 and 1M CH3COOH 1M Na2CO3. Which of the four groups IIA metal cations are definitely absent from your unknown? Please explain why.
Explore our homework questions and answers library
Browse
by subject