Question

complete the solubility table.

Explanation:

Step1: Recall solubility rules

Salts of sodium ($Na^{+}$) are generally soluble. So $NaBr$, $NaOH$, $NaClO_{4}$, $Na_{2}CO_{3}$ are soluble.

Step2: Silver - halide rule

Silver bromide ($AgBr$) is insoluble according to the solubility rules for halides.

Step3: Hydroxide solubility

Silver hydroxide ($AgOH$) is insoluble as most silver salts except nitrates, acetates and perchlorates are insoluble.

Step4: Perchlorate solubility

Perchlorates are generally soluble, so $AgClO_{4}$ is soluble.

Step5: Carbonate solubility

Silver carbonate ($Ag_{2}CO_{3}$) is insoluble as most carbonates are insoluble except those of alkali metals and ammonium.

Step6: Calcium - halide rule

Calcium bromide ($CaBr_{2}$) is soluble as calcium salts are generally soluble.

Step7: Calcium - hydroxide rule

Calcium hydroxide ($Ca(OH)_{2}$) is slightly soluble, but in general - knowledge solubility tables it is often considered soluble.

Step8: Calcium - perchlorate rule

Calcium perchlorate ($Ca(ClO_{4})_{2}$) is soluble as perchlorates are soluble.

Step9: Calcium - carbonate rule

Calcium carbonate ($CaCO_{3}$) is insoluble as most carbonates are insoluble.

Step10: Copper - halide rule

Copper(II) bromide ($CuBr_{2}$) is soluble.

Step11: Copper - hydroxide rule

Copper(II) hydroxide ($Cu(OH)_{2}$) is insoluble.

Step12: Copper - perchlorate rule

Copper(II) perchlorate ($Cu(ClO_{4})_{2}$) is soluble as perchlorates are soluble.

Step13: Copper - carbonate rule

Copper(II) carbonate ($CuCO_{3}$) is insoluble.

Answer:

The table is already completed correctly as shown in the problem statement with $Na^{+}$ compounds being soluble, $Ag^{+}$ compounds being insoluble for $Br^{-}$, $OH^{-}$, $CO_{3}^{2 -}$ and soluble for $ClO_{4}^{-}$, $Ca^{2+}$ compounds being soluble for $Br^{-}$, $OH^{-}$, $ClO_{4}^{-}$ and insoluble for $CO_{3}^{2 -}$, and $Cu^{2+}$ compounds being soluble for $Br^{-}$, $ClO_{4}^{-}$ and insoluble for $OH^{-}$, $CO_{3}^{2 -}$.